Chemistry 9 cells practical work 1. Obtaining, collecting and recognizing gases
Grade 9 Practical work No. 1. OBTAINING AMPHOTERIC HYDROXIDE AND INVESTIGATION OF ITS PROPERTIES. Progress. A) Perform experiments and complete the work. EXPERIMENT 1. Obtaining aluminum hydroxide. Pour a small amount of aluminum chloride into a test tube and add sodium hydroxide to it drop by drop. What are you watching? Record the results of the experiment in a table. Do the experiment three times. Experiment drawing Equations of reactions Conclusions EXPERIMENT 2. Interaction with acids. To the aluminum hydroxide, gently pour the solution drop by drop. nitric acid. What are you watching? Record the results of the experiment in a table. Experimental drawing Equations of reactions Conclusions EXPERIMENT 3. Interaction with alkalis. Sodium hydroxide is carefully added dropwise to the aluminum hydroxide. What are you watching? Record the results of the experiment in a table. Experimental drawing Equations of reactions Conclusions EXPERIMENT 4. Decomposition of insoluble hydroxides. Gently warm the vial of aluminum hydroxide. What are you watching? Record the results of the experiment in a table. Figure experience Reaction equations Conclusions B) Make a final conclusion on the entire work. C) Clean up the workspace.
Grade 9 Practical work No. 1. OBTAINING AMPHOTERIC HYDROXIDE AND INVESTIGATION OF ITS PROPERTIES. R E A C T I S AND EQUIPMENT. 3 test tubes, asbestos mesh, cap, matches, waste glass, fuel, test tube holder, AlCl3, NaOH, HNO3.
Grade 9 Practical work No. 2. RECOGNITION OF METAL CATIONS. Progress. A) Perform experiments and complete the work. EXPERIMENT 1. Recognition of Na + On a copper wire in a burner flame, heat a crystalline salt of sodium chloride. What are you watching? Record the results of the experiment in a table. Figure of the experiment Equations of reactions Conclusions EXPERIMENT 2. Recognition of Ca2+ Pour a solution of calcium chloride into a test tube and add a solution of sodium carbonate to it. What are you watching? Record the results of the experiment in a table. Figure of the experiment Reaction equations Conclusions EXPERIMENT 3. Recognition of Ba2+ Pour a solution of barium chloride into a test tube and add a solution of sulfuric acid to it. What are you watching? Record the results of the experiment in a table. Figure of the experiment Reaction equations Conclusions EXPERIMENT 4. Recognition of Ag + Pour a solution of hydrochloric acid into a test tube and add a drop of silver nitrate to it. What are you watching? Record the results of the experiment in a table. Experiment drawing Reaction equations Conclusions EXPERIMENT 5. Recognition of Al3+ Pour a solution of aluminum chloride into a test tube and add a solution of sodium hydroxide to it drop by drop. What are you watching? Record the results of the experiment in a table. Figure of the experiment Reaction equations Conclusions EXPERIMENT 6. Recognition of Fe2+ Pour a solution of iron chloride (II) into a test tube and add a solution of sodium hydroxide to it. What are you watching? Record the results of the experiment in a table. Drawing of the experiment Equations of reactions Conclusions EXPERIMENT 7. Recognition of Fe3+
Pour a solution of iron (III) chloride into a test tube and add a solution of sodium hydroxide to it. What are you watching? Record the results of the experiment in a table. Figure experience Reaction equations Conclusions B) Make a final conclusion on the entire work. C) Clean up the workspace. Grade 9 Practical work No. 2. RECOGNITION OF METAL CATIONS. 6 test tubes, copper wire, asbestos mesh, fuel, cap, matches, waste glass, test tube holder, NaCl (crystal), CaCl2 , Na2CO3, BaCl2, H2SO4, AgNO3, HCl, AlCl3, NaOH, FeCl2, FeCl3.
Grade 9 Practical work No. 3. IMPLEMENTATION OF CHAINS OF TRANSFORMATIONS IN PRACTICAL WAY. 1 option. CuSO4 Cu(OH)2 Cu(NO3)2 CuO Reagents and equipment: asbestos mesh, cap, fuel, matches, waste glass, test tube holder, 3 test tubes, CuSO4, NaOH, HNO3. Option 2. AlCl3 Al(OH)3 Al2(SO4)3 Na Reagents and equipment: 3 test tubes, AlCl3, NaOH, H2SO4. 3 option. FeSO4 Fe(OH)2 FeO FeCl2 Reagents and equipment: asbestos mesh, cap, fuel, matches, waste glass, test tube holder, 3 test tubes, FeSO4, NaOH, HCl. 4 option. Fe2(SO4)3 Fe(OH)3 FeCl3
Fe2O3 Reagents and equipment: asbestos mesh, cap, fuel, matches, waste glass, test tube holder, 3 test tubes, Fe2(SO4)3, NaOH, HCl. Grade 9 Practical work No. 8. RECOGNITION OF THE MOST IMPORTANT ANIONS. Progress. A) Perform experiments and complete the work. EXPERIMENT 1. Recognition of Cl Add a small amount of silver nitrate to a solution of sodium chloride. What are you watching? Record the results of the experiment in a table. Experiment drawing Reaction equations Conclusions EXPERIMENT 2. Recognition of SO4 Pour sodium sulfate solution into a test tube and add barium chloride solution to it. What are you watching? Record the results of the experiment in a table. 2 Experimental drawing Equations of reactions Conclusions EXPERIMENT 3. Recognition of CO3 Pour a solution of sodium carbonate into a test tube and add a solution of sulfuric acid to it. What are you watching? Record the results of the experiment in a table. 2 Experimental drawing Equations of reactions Conclusions EXPERIMENT 4. Recognition of PO4 Pour a solution of sodium phosphate into a test tube and add a drop of silver nitrate to it. What are you watching? Record the results of the experiment in a table. 3 Experimental drawing Equations of reactions Conclusions EXPERIMENT 5. Recognition of SiO3 Pour a solution of sodium silicate into a test tube and add a solution of sulfuric acid to it drop by drop. What do you observe? Record the results of the experiment in a table. 2
Experimental drawing Equations of reactions Conclusions EXPERIMENT 6. Recognition I Pour a solution of sodium iodide into a test tube and add a solution of silver nitrate to it. What are you watching? Record the results of the experiment in a table. Figure of the experiment Reaction equations Conclusions EXPERIMENT 7. Recognition of Br Pour a solution of sodium bromide chloride into a test tube and add a solution of silver nitrate to it. What are you watching? Record the results of the experiment in a table. Experiment drawing Reaction equations Conclusions EXPERIMENT 8. Recognition of NO3 Pour a small amount of sodium nitrate into a test tube and add a small amount of concentrated sulfuric acid and copper to it. Gently heat the test tube. What are you watching? Record the results of the experiment in a table. Experimental drawing Equations of reactions Conclusions EXPERIMENT 9. Recognition of S2 Pour a solution of sodium sulfide into a test tube and add a solution of sulfuric acid to it. What are you watching? Record the results of the experiment in a table. Experiment drawing Reaction equations Conclusions EXPERIMENT 10. Recognition of OH Drop a drop of sodium hydroxide on an indicator paper. What are you watching? Record the results of the experiment in a table. Figure experience Reaction equations Conclusions B) Make a final conclusion on the entire work. C) Clean up the workspace.
Grade 9 Practical work No. 8. RECOGNITION OF THE MOST IMPORTANT ANIONS. 9 test tubes, indicator paper, glass of water, glass rod, asbestos mesh, fuel, matches, waste glass, cap, test tube holder, NaCl , Na2SO4, Na2CO3, Na3PO4, Na2SiO3, NaI, NaBr, NaNO3, Na2S, NaOH, AgNO3, BaCl2, H2SO4, H2SO4 (conc.), Cu.
Grade 9 Practical work No. 9. SOLUTION OF EXPERIMENTAL PROBLEMS. Experience 1. Obtain copper (II) nitrate in two different ways. Write the reaction equations in molecular and ionic forms. Record the results of the experiments in a table. Experiment drawing Reaction equations Conclusions Experiment 2. Prove the qualitative composition of acids: 1st option: hydrochloric acid 2nd option: sulphuric acid 3 option: phosphoric acid. Write the reaction equations in molecular and ionic forms. Record the results of the experiment in a table.
Drawing of the experiment Reaction equations Conclusions Experience 3. In a practical way to carry out a chain of transformations: Mg Write down the reaction equations in molecular and ionic forms. Record the results of the experiments in a table. Mg(OH) MgCl Mg(NO 3)2 → 2 → → 2 Figure of experience Reaction equations Conclusions Make a final conclusion on the work. Clean up the workplace. Grade 9 Practical work No. 9. SOLUTION OF EXPERIMENTAL PROBLEMS. O O R U D O V A N I E AND R E A C T I V Y. CuO, HNO3, CuCl2, NaOH, Mg, HCl, option 1: indicator paper, glass of water, glass rod, AgNO3. Option 2: indicator paper, glass of water, glass rod, BaCl2, H2SO4. Option 3: indicator paper, glass of water, glass rod, AgNO3, H3PO4.
Practical work No. 1
on this topic: "»
Objective:
Equipment:
Progress
1. Tripod device
2. Spirit lamp device
3.Dishes
4.Filtering
3. put into the funnel;
"8th grade"
Practical work No. 1
on this topic: "Safety rules for working in a chemical laboratory. Techniques for handling laboratory equipment and heating devices»
Safety briefing.
Objective: Familiarize yourself with the device and the basic methods of handling laboratory equipment.
Equipment: Tripod, spirit lamp, laboratory glassware.
Progress
1. Tripod device(draw a tripod, identify its components)
2. Spirit lamp device(draw a spirit lamp, designate its components)
3.Dishes(draw test tubes, flasks, beaker)
4.Filtering
1. prepare filter paper;
2. moisten the filter paper;
3. put into the funnel;
4. the liquid is poured over a glass rod, directing it to the wall of the funnel;
5. the filtrate flows down the wall of the glass, and not into the center, so that it does not splash out.
Find in the text the definitions of filtrate, sediment and filtration process.
Practical work №2
on this topic: « Observations of the changes that occur with a burning candle, and their description»
Target: observe physical and chemical phenomena during the burning of a candle.
Equipment: glass slide, candle, matches, dry test tube, holder.
Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
The test tube is fixed in the holder so that there is a distance of 1–1.5 cm from the neck of the test tube to the holder.
The glass slide is first heated completely, and then brought into the zone of the dark cone of a burning candle.
First aid for burns:
First aid for cuts:
Experience number 1. physical phenomena while burning a candle.
Light a candle. You will see how the paraffin near the wick begins to melt, forming a round puddle. What process is taking place here?
Experience number 2. Detection of combustion products in a flame.
Take a glass slide, fix it in the holder ( t/b), bring a burning candle into the zone of the dark cone and hold for 3-5 s. Quickly raise the glass, look at the bottom plane. Explain what happened there.
Fix the dry test tube in the holder ( t/b), turn upside down and hold over the flame until fogging. Explain the observed phenomenon.
Practical work No. 3
on this topic: "Soil and water analysis»
Target: determine the composition of the soil, learn how to filter and evaporate the liquid.
Equipment: two test tubes, a funnel, a paper filter, a glass rod, a glass slide, a spirit lamp, a glass cylinder with water, a stopper, universal indicator paper.
Safety instructions:
The glass slide is fixed in the holder at one of its edges neatly. This takes into account that glass is a fragile material and can crack if it is pressed hard.
In the process of evaporating water from the soil extract, the entire glass slide is first heated, and then a drop of liquid on it.
First aid for cuts:
a) first of all, it is necessary to stop the bleeding (pressure bandage, clamping of the vessel);
b) if the wound is contaminated, the dirt is removed only around it, but in no case - from the deep layers of the wound. The skin around the wound is disinfected with iodine tincture or brilliant green solution;
c) after treatment, the wound is covered with a sterile napkin so as to cover the edges of the wound, and tightly bandaged with a regular bandage;
d) after receiving first aid, go to the first-aid post.
First aid for burns:
A first-degree burn is treated with ethyl alcohol, then, to relieve pain, glycerin and a dry sterile bandage is applied. In all other cases, a sterile bandage is applied after the burn site has cooled and the patient is referred to a first-aid post.
Experience number 1. Mechanical analysis of the soil.
Soil is placed in a test tube. Pour water to it, the volume of which should be 3 times the volume of the soil. Stopper the tube and shake vigorously for 1-2 minutes. Observe the precipitation of soil particles and the structure of precipitation. Describe and explain your observations.
Experience number 2. Obtaining a soil solution and experiments with it.
Prepare a paper filter, insert it into a clean test tube and filter the mixture of soil and water obtained in the first experiment. The mixture should not be shaken before filtering. The soil will remain on the filter, and the filtrate collected in the test tube is a soil extract (soil solution).
Place a few drops of this solution with a glass rod on a glass slide and hold it over the flame of an alcohol lamp ( t/b) until the water evaporates. What are you watching? Explain.
Take a universal indicator paper, put a soil solution on it with a glass rod. Make a conclusion based on your observations.
Practical work No. 4
on this topic: "Preparation of a sugar solution and determination of its mass fraction in solution»
Safety briefing
Target: learn how to weigh on a laboratory scale, determine the volume of a liquid using a measuring cylinder, prepare a solution with a certain mass fraction of a substance.
Equipment and reagents: beaker, stirring stick, measuring cylinder, laboratory scales, weights; sugar, water.
Work order
Calculate the mass of sugar and mass of water required to prepare the solution you need using the formulas:
m (substances) =m (solution) ω(substance)
m
(H
2
O
) =
m
(solution) -m
(substances)
Calculations give in the report on practical work.
Determine the volume of water corresponding to the calculated mass using the formula: V =m
· ρ.
Remember that for water ρ = 1 g/ml.
Give the calculation in the report on practical work.
Use a graduated cylinder to measure the calculated volume of water. Pour the water into a beaker.
Weigh the calculated mass of sugar on a laboratory scale. Pour sugar into a glass of water.
Stir the contents of the beaker until the sugar is completely dissolved.
Draw a conclusion about what is needed to prepare a solution with a certain mass fraction of a solute.
Practical work No. 5
on this topic: "Signs of chemical reactions»
Target: consider examples of chemical reactions and identify their signs.
Equipment: test tubes, copper wire, spirit lamp, copper (II) oxide, sulfuric acid solution, marble, hydrochloric acid solution, iron (III) chloride and potassium thiocyanate solutions, sodium sulfate and barium chloride solutions.
Safety instructions:
If you light the spirit lamp immediately after removing the cap, a film of alcohol on the neck of the spirit lamp lights up just at the place where the cap is adjacent to the neck. The flame penetrates under the disk with the tube, and the alcohol vapor inside the tank ignites. There may be an explosion and ejection of the disc along with the wick. To avoid this, lift the disc with the wick for a few seconds to remove the fumes. If the fumes ignite, quickly set aside the objects (notebook for practical work) and call the teacher.
A lit spirit lamp must not be moved from place to place, nor can one kind of spirit lamp be lit directly from another. Use matches to light a spirit lamp.
There is only one way to extinguish the spirit lamp - to cover the flame of the wick with a cap. The cap should always be at hand.
Acids are corrosive substances. Destroy and irritate the skin, mucous membranes.
It is necessary to pour the acid in such a way that when the bottle is tilted, the label, in order to avoid damage to it, is on top.
Copper compounds in the form of dust upon contact with the skin, especially in places of microtrauma, can cause irritation, lead to mild allergies.
Barium compounds must be handled in such a way as to prevent them from getting into the mouth, as they are toxic. To obtain severe poisoning, a dose weighing less than 0.5 g is sufficient. After finishing work, wash your hands thoroughly with soap and running water.
First aid for cuts:
a) first of all, it is necessary to stop the bleeding (pressure bandage, clamping of the vessel);
b) if the wound is contaminated, the dirt is removed only around it, but in no case - from the deep layers of the wound. The skin around the wound is disinfected with iodine tincture or brilliant green solution;
c) after treatment, the wound is covered with a sterile napkin so as to cover the edges of the wound, and tightly bandaged with a regular bandage;
d) after receiving first aid, go to the first-aid post.
First aid for burns:
A first-degree burn is treated with ethyl alcohol, then, to relieve pain, glycerin and a dry sterile bandage is applied. In all other cases, a sterile bandage is applied after the burn site has cooled and the patient is referred to a first-aid post.
First aid in case of acid contact with the skin of the hands:
Shake off drops of acid that have fallen on the skin and rinse thoroughly with plenty of water, and then treat the affected surface with a 2% solution of baking soda.
First aid for poisoning with barium salts:
Rinse the stomach with 1% sodium sulfate or magnesium sulfate solution.
Experience No. 1 Calcination of copper wire.
Light up the alcohol lamp. Take a copper wire with crucible tongs and bring it into the flame. After a while, remove the wire from the flame. What are you watching?
Experiment No. 2 Interaction of sodium carbonate with hydrochloric acid.
Put some sodium carbonate into a small beaker. Pour enough hydrochloric acid into the beaker to cover the sodium carbonate. What are you watching?
Light a torch and put it into a glass. What are you watching?
Make a report by filling in the table.
Experiment No. 3 Interaction of ammonium chloride with sodium hydroxide.
Put some ammonium chloride into the test tube. Pour enough sodium hydroxide solution into the test tube to cover the ammonium chloride with it. Shake well. Carefully sniff the contents of the vial.
Make a report by filling in the table.
Experiment No. 4 Interaction of copper sulfate ( II ) with sodium hydroxide.
Pour 2 ml of sodium hydroxide solution into a test tube, and then add 2-3 drops of copper (II) sulfate to it. What are you watching?
Make a report by filling in the table.
Experiment No. 5 Interaction of copper hydroxide ( II ) with hydrochloric acid.
Add a small amount of hydrochloric acid to copper (II) hydroxide. Shake gently. What are you watching?
Make a report by filling in the table.
Experience No. 6 Burning alcohol
Pour 2 ml of ethyl alcohol into a cup. Set it on fire carefully. What are you watching? Make a report by filling in the table.
Experience No. 7 Decomposition of malachite
Pour a small amount of malachite into a test tube. Heat it up in the flame of an alcohol lamp. What are you watching?
Make a report by filling in the table.
| What they were doing | Observations | (feature chemical reaction) |
Practical work No. 6
on this topic: "Properties of acids, bases, oxides and salts»
Target: to put into practice reactions characterizing the properties of acids, bases, oxides and salts.
Equipment and reagents: rack with test tubes; sulfuric acid, phosphoric acid, zinc, iron, copper(II) oxide, sodium hydroxide, silver nitrate, barium chloride, sodium carbonate, sodium phosphate, copper(II) chloride, phenolphthalein
Safety briefing:
Progress
| What they were doing | |
| Experience 1 |
|
| Experience 2 |
|
Work order
Experience 1. Carry out reactions characterizing the properties of a sulfuric acid solution:
a) acid + metal = salt + H 2
b) acid + basic oxide \u003d salt + H 2 O
c) acid + base = salt + H 2 O
d) acid + salt \u003d salt + acid
Experience 2. Perform reactions characterizing the properties of copper chloride (II):
a) salt + metal \u003d salt + metal
b) salt + alkali \u003d base ↓ + salt
c) salt + acid \u003d salt + acid
d) salt + salt \u003d salt + salt ↓
Make up the equations of the reactions performed in molecular and ionic form.
Practical work number 7
on this topic: "Solution of experimental problems»
Target: to carry out the set tasks experimentally.
Equipment and reagents: rack with test tubes; copper(II) sulfate, sodium hydroxide, barium chloride, sodium sulfate, magnesium sulfate, sodium carbonate, hydrochloric acid, phenolphthalein
Safety briefing
Progress
| What they were doing | Observations and equations of chemical reactions | Conclusion about the type of chemical reaction |
| Experience 1. |
||
| Experience 2. |
||
Work order
Experience 1. Carry out the reactions, the schemes of which are given:
a) Ba 2+ + SO 4 2- \u003d BaSO 4
b) CO 3 2- + 2H + = H 2 O + CO 2
c) OH - + H + \u003d H 2 O
In the table, write down the observations and reaction equations in molecular complete and abbreviated and ionic form.
Experience 2. Using the solutions on the table, get:
a) copper hydroxide (II)
b) magnesium carbonate
Record your observations in a table. Write reaction equations in molecular, full and reduced ionic form.
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"Grade 9"
Practical work No. 1
on this topic: "Implementation of a chain of chemical transformations»
Safety briefing.
Objective: Solution of experimental problems consisting of a chain of transformations.
Equipment: Rack with test tubes.
Reagents (1st century): Magnesium sulfate MgSO 4 , alkali NaOH , barium chloride BaCl 2 .
Reagents (2v.): Copper sulfate CuSO 4, alkali NaOH, hydrochloric acid HCl, Fe (paper clip).
Option 1: MgSO 4 - MgCl 2 - Mg (OH) 2 - MgSO 4
| Reaction equations | ||
| MgSO4+ Mg 2+ + SO 4 2- + | ||
| MgCl 2 + Mg 2+ + 2Cl - + | ||
| Mg (OH) 2 + |
Conclusion:
Option 2: CuSO 4 -Cu (OH) 2 - CuO - Cu
| Reaction equations | ||
| CuSO4+ | ||
| Cu (OH) 2 | ||
| CuO+ |
Conclusion:
Practical work No. 2
This appendix contains instructions for practical work for 9th grade students.
"Practical work No. 1 - 9 cells"
| Practical work No. 1 Objective: Empirically prove the amphotericity of aluminum. Prove the qualitative composition of CaCO 3. Equipment: Rack with test tubes. Reagents: Option 1 Exercise 1.
Conclusion: Task 2
Conclusion: Task3. Prove the qualitative composition of CaCL 2
Conclusion: | Practical work No. 1 Preparation of metal compounds and study of their properties Safety briefing. Objective: Empirically prove the amphotericity of aluminum. Prove the qualitative composition of FeSO 4. Equipment: Rack with test tubes. Reagents: AlCl 3, NaOH, HCl, FeSO 4, BaCl 2, K 3. Option 2 Exercise 1. Determine whether the result of the reaction depends on the order in which the reactants are poured.
Conclusion: Task 2. Investigation of the properties obtained by Al (OH)3.
Conclusion: Task3. Prove the qualitative composition of FeSO 4
Conclusion: |
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"Practical work No. 2 - 9 cells"
| Practical work №2 Safety briefing. Objective: Solution of experimental problems consisting of a chain of transformations. Equipment: Rack with test tubes. Reagents Option 1: MgSO 4 - MgCl 2 - Mg (OH) 2 - MgSO 4
Conclusion: | Practical work №2 Implementation of a chain of chemical transformations of metals Safety briefing. Purpose of work s: Solution of experimental problems consisting of a chain of transformations. Equipment: Rack with test tubes. Reagents: Copper sulfate CuSO 4, alkali NaOH, hydrochloric acid HCl, Fe (paper clip). Option 2: CuSO 4 -Cu (OH) 2 - CuO - Cu
Conclusion: |
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"Practical work No. 3 - 9 cells"
| Practical work No. 3 Safety briefing. Objective Equipment: Reagents Progress Exercise 1. Task2. 4 . Task 3. |
| Practical work No. 3 Solving experimental problems on the topic "Oxygen subgroup" Safety briefing. Objective: To consolidate the theoretical knowledge of qualitative reactions in practice. Equipment: Stand with test tubes, cup for evaporation, holder, spirit lamp. Reagents: Indicator phenolphthalein, AgNO 3 , BaCl 2 , NaOH , H 2 SO 4 , HCl , NaCl , KI , ZnSO 4 . Progress Exercise 1. Determine in which test tube which of the substances is NaOH, H 2 SO 4, HCl. Task2. Give qualitative reactions for substances NaCl , KI , ZnSO 4 . Task 3. Get from CuO , CuSO 4 , and CuSO 4 ∙5H 2 O . |
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"Practical work No. 5 -9 cells"
Practical work No. 5.
Obtaining carbon monoxide ( IV ) and study its properties.
Objective: _________________________________________________________________
_____________________________________________________________________
Equipment: ________________________________________________________________
Reagents:
| Name | |
| Hydrochloric acid | |
| lime water | |
| Sodium carbonate |
Precautionary measures: _____________________________________________________________
_____________________________________________________________________________________
Progress: Arrange the results of the work in the form of a table
| Name of experience | What they were doing? | What did you observe? | chemical reaction equation (in molecular, full, abbreviated ionic form) |
| Obtaining carbon dioxide and studying its properties | CaCO 3 + HCl = H 2 O + CO 2 ↔ H 2 CO 3 + Ca(OH) 2 = |
||
| Experience number 2. Interconversion of carbonates and hydrocarbonates | CO 2 + Ca (OH) 2 \u003d CaCO 3 + CO 2 + H 2 O ↔ Ca(HCO 3 ) 2 t˚C → |
||
| Experience number 3. Recognition of carbonates | Na 2 CO 3 + HCl \u003d |
Conclusion (fill the gaps):
Carbon monoxide (IV) in the laboratory can be obtained ____________________________________________
_____________________________________________________________________________________
The following properties of CO 2 have been found:
Physical __________________________________________________________________________Chemical __________________________________________________________________________
_____________________________________________________________________________________
When carbon dioxide is passed through lime water, _____________ calcium carbonate is first formed, which is ________________ in excess of carbon dioxide.
Calcium bicarbonate thermally ____________________, when heated _______________ to form ______________________.
All carbonates can react with ________________ acids to form _________________, this reaction is __________________________________________________________________________________.
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"Practical work No. 4 -9 cells"
Practical work No. 4. (Grade 9)
Topic:"Obtaining ammonia and studying its properties"
Purpose: Get ammonia and get acquainted with the properties aqueous solution ammonia.
Equipment and reagents:
Instructions for performing practical work.
Repeat the textbook questions: obtaining and properties of ammonia, ammonia water and ammonium salts. After that, get to work.
Experience number 1. Getting ammonia .
Assemble the device for obtaining ammonia.
Pour four spatulas of ammonium chloride and two spatulas of calcium hydroxide into a porcelain cup. Stir the mixture with a spatula and pour into a dry test tube. Close it with a stopper with a gas outlet tube and fix it in the leg of the tripod (pay attention to the inclination of the test tube with the mixture). Put a dry tube to collect ammonia on the gas outlet tube and close its opening with a cotton swab.
Heat a test tube with a mixture of ammonium chloride and calcium hydroxide slightly (2-3 flame movements), and then heat in the place where the mixture is located. To detect ammonia, place a wet phenolphthalein paper upside down in a test tube. Having found ammonia, bring a glass rod moistened with a solution of hydrochloric acid to the opening of the test tube. What are you watching? What chemical composition generated particulate matter (smoke)? Write the reaction equation.
Stop heating the mixture. Carefully remove the test tube in which ammonia is collected from the gas outlet tube, holding it upside down (immediately after removing the test tube with ammonia from it, close the end of the gas outlet tube with a piece of wet cotton wool).
Immediately close the opening of the removed test tube with your thumb and lower it into a vessel of water. Remove your finger only under water. What are you watching? Why did the water rise in the test tube? Close the opening of the tube under water again with your finger and remove it from the vessel.
Answer the questions
1. Why does a test tube with a mixture of substances for ammonia production need to be fixed in the leg of a tripod at an angle with a raised bottom?
2. Why is ammonia collected in a tube turned upside down? What other gases can be collected in this way?
3. How can you prove that an aqueous solution of ammonia contains hydroxide ions?
With the resulting aqueous solution of ammonia, do the following experiments.
Studying the properties of an aqueous solution of ammonia
Experience number 1. Pour 2-3 ml of an aqueous ammonia solution into a test tube and add 2-3 drops of phenolphthalein. What is the color of the solution? Heat this solution to a boil. How will the color of the solution change? What caused this change?
Experience number 2. Pour 2-3 ml of an aqueous ammonia solution into a test tube. Add 2-3 drops of phenolphthalein and add sulfuric acid solution drop by drop until the crimson color disappears. Why is the color gone? Write the ionic equations for the reaction.
Write a work report. Make a conclusion.
| The name of the experience. | Observations. Drawings. | Reaction equations | |
All video experiments on this work can be viewed on the Digital Educational Resources website.
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"Practical work grade 9 equipment and reagents"
Practical work Grade 9
| Job title | Equipment and reagents |
|
| Preparation of metal compounds and study of their properties | Equipment: Rack with test tubes. Reagents: AlCl 3, NaOH, HCl, CaCL 2, AgNO 3. |
|
| Implementation of a chain of chemical transformations of metals | Equipment: Rack with test tubes. Reagents: Magnesium sulfate MgSO 4 , alkali NaOH , barium chloride BaCl 2 . |
|
| Oxygen subgroup | Equipment: Stand with test tubes, cup for evaporation, holder, spirit lamp. Reagents: Indicator phenolphthalein, AgNO 3 , BaCl 2 , NaOH , H 2 SO 4 , HCl , NaCl , KI , ZnSO 4 . |
|
| Obtaining ammonia and studying its properties | Equipment and reagents: spirit lamp, metal stand, cork with a gas outlet tube, spatula, porcelain cup, glass rod, 5 test tubes, cotton swab, crystallizer half-filled with water, phenolphthalein paper; ammonium chloride, calcium hydroxide, ammonia solution (1%), sulfuric acid solution (1:5), hydrochloric acid solution (1:3). |
|
| Obtaining carbon dioxide, studying its properties | Equipment: rack with test tubes, stopper with vent tube Reagents: marble, hydrochloric acid, lime water, sodium carbonate |
Practical work №1.
Influence of various factors on the rate of a chemical reaction.
Target: consider the influence of various factors on the rate of a chemical reaction.
Equipment and reagents:test tubes, spirit lamp, holder, test tube stand, zinc, magnesium, iron: granules and powder, solutions of sulfuric (1:5, 1:10) and hydrochloric acid, hydrogen peroxide, manganese (IV) oxide, copper (II) oxide.
Progress:
EXPERIMENT 1. Influence of the nature of reacting substances.
EXPERIMENT 2. Influence of the concentration of reactants.
EXPERIMENT 3. Influence of the contact area of reactants.
EXPERIMENT 4. Effect of temperature.
Place a little black powder of copper oxide (II) in de test tubes, pour a solution of sulfuric acid into both test tubes. Heat one of the tubes
EXPERIMENT 5. Influence of the catalyst.
2 O 2 2 . In which tube is the reaction faster? Why?
Organize your work in a table:
The considered factor influencing the rate of chem. reactions | Description of the experiment | Observations to judge the rate of a reaction | Reaction equations | Conclusion |
Experience 1. Influence of the nature of reacting substances. | Pour 2 ml of hydrochloric acid solution into three test tubes. Put a piece of magnesium in the first glass, a zinc granule in the second glass, and a piece of iron in the third glass. Observe the rate of the three reactions. Which reaction is the fastest and why? | Gas evolution occurs most rapidly in a test tube with magnesium. | Mg + 2HCl → MgCl 2 + H 2 Zn + 2HCl → ZnCl 2 + H 2 Fe + 2HCl → FeCl 2 + H 2 | The rate of a chemical reaction depends on the nature of the reactants. Magnesium has the strongest reducing properties. |
Experience 2. Influence of the concentration of reactants. | In two test tubes, tilting them, lower a zinc granule, carefully pour sulfuric acid solutions: in the first test tube, an acid solution of 1:5, in the second - 1:10. Which one reacts faster? | In the first tube, the gas is released more intensively. | Zn + H 2 SO 4 → ZnSO 4 + H 2 | The higher the concentration of the reactants, the more frequent the collisions of their particles and the higher the rate of the chemical reaction. |
Experience 3. Influence of the contact area of reactants. | Pour a little iron powder into one test tube, put an iron clip into the other, and pour 2 ml of dilute hydrochloric acid (1: 2) into both test tubes.In which tube is the reaction faster? Why? | The evolution of gas is faster in a test tube with iron powder. | Fe + 2HCl → FeCl 2 + H 2 | The larger the contact area of the reactants, the higher the rate of the chemical reaction. |
Experience 4. The effect of temperature. | Place a little black powder of copper (II) oxide into two test tubes, pour a solution of sulfuric acid into both test tubes. Heat up one of the test tubes. In which tube is the reaction faster? Why? | The dissolution of copper oxide (II) and the formation of a blue solution is faster when heated. | СuO + H 2 SO 4 CuSO 4 + H 2 O | As the temperature rises, the speed of particle movement and the rate of the chemical reaction increase. |
Experience 5. Influence of the catalyst. | Pour 2 ml of hydrogen peroxide H into two test tubes. 2 O 2 , add a few crystals of manganese (IV) oxide MnO to one of the test tubes 2 . In which tube is the reaction faster? Why? | In the presence of manganese (IV) oxide, there is a rapid release of gas bubbles. | 2H 2 O 2 2H 2 O + O 2 | Manganese (IV) oxide is a catalyst that accelerates the decomposition of hydrogen peroxide. |
Conclusion: The rate of a chemical reaction depends on the conditions: on the nature of the reactants, on the contact area, on the concentration, on the temperature, on the presence of catalysts.
Practical work №2.
Solving experimental problems on the topic "Electrolytic dissociation".
Target: learn to apply theoretical knowledge for experimental problem solving.
Equipment and reagents:test tubes, solutions of sulfuric acid, sodium chloride, sodium sulfate, hydrochloric acid, silver nitrate, barium chloride, indicators, copper (II) sulfate, sodium hydroxide.
Progress:
Remember the safety rules when performing a chemical experiment.
- Many substances can cause burns if they come into contact with the skin. Never handle substances with your hands.
- Some substances have an unpleasant odor, and their vapors can cause poisoning. Do not bring an open bottle close to your face.
- In a chemical laboratory, even known substances are not tasted, they may contain impurities that are toxic to humans.
- Acids are corrosive substances. Destroy and irritate the skin, mucous membranes.
- If acid or alkali gets on the skin, it should be washed immediately with plenty of running water.
- Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
- Experiments should be carried out with the amount of substances indicated in the methodological manual for each experiment.
- Without the permission of the teacher, do not touch anything on the tables.
- Maintain silence while conducting an experiment or writing a report.
- Clean up your workspace after work.
Task number 1. Determine empirically the composition of solutions that are without labels: sulfuric acid, sodium chloride, sodium sulfate.
Substance reagent | H 2 SO 4 | NaCl | Na2SO4 |
litmus | Red color | no change | no change |
BaCl2 | no change | BaSO4 ↓ White |
|
AgNO3 | AgCl↓ white curdled | ||
tube number: |
H 2 SO 4 → 2H + + SO 4 2-
Ba 2+ + SO 4 2- → BaSO 4 ↓
NaCl + AgNO 3 → NaNO 3 + AgCl↓
Ag + + Cl - → AgCl ↓
Task number 2. Confirm the qualitative composition of substances:
1) Hydrochloric acid.
Hydrochloric acid dissociates into ions:НCl → H + + Cl -
A qualitative reaction to the hydrogen cation is litmus. A red color is formed.
A qualitative reaction to the chloride anion is interaction with silver nitrate, a white cheesy precipitate is formed.
НCl + AgNO 3 → НNO 3 + AgCl↓
Ag + + Cl - → AgCl ↓
2) Copper sulfate (II).
Copper sulfate (II) dissociates into ions: CuSO 4 → Cu 2+ + SO 4 2-
Qualitative reaction to sulfate ion - interaction with barium chloride. A white precipitate of barium sulfate is formed:
CuSO 4 + BaCl 2 → CuCl 2 + BaSO 4 ↓
Ba 2+ + SO 4 2- → BaSO 4 ↓
Qualitative reaction to the copper cation Cu 2+ - interaction with sodium hydroxide solution. A blue gelatinous precipitate of copper (II) hydroxide is formed:
CuSO 4 + 2NaOH → Na 2 SO 4 + Cu(OH) 2 ↓
Cu 2+ + 2OH - → Cu(OH) 2 ↓
Conclusion:
Practical work №3.
Obtaining ammonia and the study of its properties. Familiarization with chemical properties aqueous solution of ammonia.
Target: 1. To consolidate the ability to receive gases and collect them, taking into account the relative density in the air.
2. To study the properties of ammonia and ammonia water, learn how to obtain and recognize ammonium salts.
Equipment and reagents:laboratory tripod, spirit lamp, cork with a vent tube, spatula, porcelain mortar with pestle, crystallizer with water, splinter, cotton swab, test tubes, litmus paper, ammonium chloride, ammonium sulfate, calcium hydroxide, 1% ammonia solution, solutions of hydrochloric and sulfuric acids , sodium hydroxide.
Progress:
Remember the safety rules when performing a chemical experiment.
- Many substances can cause burns if they come into contact with the skin. Never handle substances with your hands.
- Some substances have an unpleasant odor, and their vapors can cause poisoning. Do not bring an open bottle close to your face.
- In a chemical laboratory, even known substances are not tasted, they may contain impurities that are toxic to humans.
- Acids are corrosive substances. Destroy and irritate the skin, mucous membranes.
- Alkalis are caustic substances. Destroy and irritate the skin, mucous membranes. They can cause complete loss of vision.
- If acid or alkali gets on the skin, it should be washed immediately with plenty of running water.
- Ammonia requires careful handling due to its physiological activity, it affects the respiratory tract (dehydration).Ammonia, which will be released during the interaction of ammonium salts with alkalis, is very soluble in water, and hence in the moisture of the mucous membrane of the eyes. They may become irritated. If this happens, rinse eyes with water.
- If you light the spirit lamp immediately after removing the cap, a film of alcohol on the neck of the spirit lamp lights up just at the place where the cap is adjacent to the neck. The flame penetrates under the disk with the tube, and the alcohol vapor inside the tank ignites. There may be an explosion and ejection of the disc along with the wick. To avoid this, lift the disc with the wick for a few seconds to remove the vapors. If a fumes ignite, quickly put things aside (practical workbook) and call the teacher.
- Light the spirit lamp only with matches, extinguish with a lid or cap, covering from above.
- It is forbidden to transfer a lit spirit lamp and to light one spirit lamp from another.
- When heating a substance in a test tube, it must first be heated; the opening of the test tube during heating should be directed away from itself and its neighbor.
- Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
- Experiments should be carried out with the amount of substances indicated in the methodological manual for each experiment.
- Without the permission of the teacher, do not touch anything on the tables.
- Maintain silence while conducting an experiment or writing a report.
- Clean up your workspace after work.
Page 116-117
Name of experience | What they were doing | Observations, drawings | Reaction equations | Conclusion |
Experience 1. Receiving ammonia and dissolving it in water. | In a porcelain mortar, mix equal volumes of solid ammonium chloride NH 4 Cl and calcium hydroxide Ca(OH) 2 . Pour the prepared mixture into a test tube to 1/3 of its volume. Close the test tube with a stopper with a gas outlet tube. Mount the tube at an angle so that the bottom is slightly higher than the stopper. Explain why? Put a dry test tube on the end of the gas outlet tube, closing the hole from the bottom with a cotton swab. Heat the mixture: first the entire tube, then the reaction mixture. Why is ammonia collected in a tube turned upside down? When you smell ammonia, plug the test tube with your finger and, without turning it over, immerse it in a crystallizer with water. What are you observing? What caused this phenomenon? Invert the test tube with the solution, test with phenolphthalein. What are you observing? Make a conclusion. | figure ris1.jpg Water vapor condenses at the cork. There is a smell of ammonia. Rapid suction of water into the test tube. The appearance of crimson color. | Ca (OH) 2 + 2NH 4 C1 CaC1 2 + 2NH 3 + 2H 2 O NH 3 + H 2 O ⇄ NH 3 H 2 O ⇄ NH 4 + +OH - | The neck of the test tube is tilted slightly downwards so that drops of water do not flow onto the warmer walls of the test tube, otherwise it may crack. Ammonia is a gas, almost 2 times lighter than air, so it is collected in a test tube turned upside down. Ammonia dissolves very well in water, a vacuum is created in the test tube. The medium is alkaline. |
Experience 2. The interaction of ammonia with acids. | Lower the gas outlet tube into test tubes ¼ filled with hydrochloric acid and sulfuric acid solutions. What are you observing? | Above the surface of acid solutions, “white smoke” appears - crystalline chloride and ammonium sulfate. | NH 3 + HCl → NH 4 Cl NH 3 + H 2 SO 4 → (NH 4) 2 SO 4 | Ammonia actively reacts with acids. |
Experience 3. Interaction of ammonium salts with alkalis (recognition of ammonium salts) | Place a little crystalline ammonium sulfate in a test tube, add 2 ml of sodium hydroxide solution, heat slightly. What do you feel? Hold a wet litmus paper up to the opening of the test tube. What are you observing? Conclude how to recognize ammonium salts. | A gas with a pungent odor is released. She turns blue. | (NH 4) 2 SO 4 + 2NaOH → Na 2 SO 4 + 2NH 3 + 2H 2 O NH 3 + H 2 O ⇄ NH 3 H 2 O ⇄ NH 4 + +OH - | The medium is alkaline. A qualitative reaction to ammonium salts is their interaction with alkalis when heated. |
Conclusion: We studied the properties of ammonia, learn how to obtain and recognize ammonium salts.
Practical work No. 4.
Preparation of carbon monoxide (IV) and study of its properties. Recognition of carbonates.
Target: 1. Consolidate knowledge about the properties of carbon dioxide and carbonates.
2. Learn to receive carbon dioxide exchange reaction and recognize it.
Equipment and reagents:laboratory tripod, cork with a gas outlet tube, chemical beaker, test tubes, litmus, solutions of hydrochloric acid, sodium chloride, sodium carbonate, sodium sulfate, barium chloride, silver nitrate, marble, lime water.
Progress:
Remember the safety rules when performing a chemical experiment.
- In a chemical laboratory, even known substances are not tasted, they may contain impurities that are toxic to humans.
- Acids are corrosive substances. Destroy and irritate the skin, mucous membranes.
- If acid or alkali gets on the skin, it should be washed immediately with plenty of running water.
- Barium compounds must be handled in such a way as to prevent them from getting into the mouth, as they are toxic. To obtain severe poisoning, a dose weighing less than 0.5 g is sufficient. After finishing work, wash your hands thoroughly with soap and running water.
- Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
- The test tube is fixed in the holder so that there is a distance of 1–1.5 cm from the neck of the test tube to the holder.
- Experiments should be carried out with the amount of substances indicated in the methodological manual for each experiment.
- Without the permission of the teacher, do not touch anything on the tables.
- Maintain silence while conducting an experiment or writing a report.
- Clean up your workspace after work.
Experience 1 . Preparation of carbon monoxide (IV) and study of its properties. Page 158-159
What they were doing | Observations, drawings | Reaction equations | Conclusion |
Assemble the apparatus for obtaining gases. Check it for tightness. Place a few pieces of marble in a test tube and add 2 ml of dil. of hydrochloric acid. What are you observing? Close the test tube with a cork with a gas outlet tube and pass the released gas through lime water. What do you are you watching? Continue to pass gas for a few minutes. What are you observing? Place the end of the gas tube in a test tube with 2-3 ml of distilled water and a few drops of litmus and pass carbon dioxide through it. What are you observing? | figure ris2 Violent release of gas. Turbidity of lime water. The formed precipitate dissolves. Litmus blushes. | CaCO 3 + 2HCl → CaCl 2 + CO 2 + H 2 O CaCO 3 + 2H + →Ca 2+ + CO 2 + H 2 O CO 2 + Ca(OH) 2 → CaCO 3 ↓ + H 2 O CaCO 3 + H 2 O + CO 2 → Ca(HCO 3 ) 2 CaCO 3 + H 2 O + CO 2 → Ca 2+ + 2HCO 3 - CO 2 + H 2 O ↔ H 2 CO 3 | In the laboratory, carbonates are treated with a strong acid to produce carbon dioxide. Lime water is used to detect carbon dioxide. With an excess of carbon dioxide, insoluble carbonates turn into soluble hydrocarbons. When carbon dioxide dissolves, it forms carbonic acid, then. carbon dioxide is an acidic oxide. |
Conclusion: 1. In the laboratory, carbon dioxide is produced by the action of hydrochloric acid on carbonates.
2. A qualitative reaction to carbon dioxide is the turbidity of lime water.
Experience 2 . Recognition of carbonates.
Three test tubes contain solutions of the following substances: sodium chloride, sodium sulfate, sodium carbonate. Recognize these substances by determining the sequence of operations.
Substance reagent | NaCl | Na2SO4 | Na2CO3 |
no change | no change | "boiling" CO 2 |
|
BaCl2 | no change | BaSO4 ↓ White | |
AgNO3 | AgCl↓ white curdled | ||
tube number: |
Na 2 CO 3 + 2HCl → 2NaCl + CO 2 + H 2 O
2H + + CO 3 2- → CO 2 + H 2 O
Na 2 SO 4 + BaCl 2 → 2NaCl + BaSO 4 ↓
Ba 2+ + SO 4 2- → BaSO 4 ↓
NaCl + AgNO 3 → NaNO3 + AgCl↓
Ag+ +Cl- → AgCl ↓
Conclusion:1. Substances can be recognized using qualitative reactions.
2. Qualitative reaction to the carbonate ion - the interaction of carbonates with strong acids.
Practical work No. 5.
Determination of the qualitative composition of organic matter.
Target:learn to experimentally determine the qualitative composition of organic substances.
Equipment and reagents:laboratory tripod, spirit lamp, cork with a gas outlet tube, test tubes, anhydrous copper (II) sulfate, copper (II) oxide, vaseline, lime water.
Progress:
Remember the safety rules when performing a chemical experiment.
- Alkalis are caustic substances. Destroy and irritate the skin, mucous membranes. They can cause complete loss of vision.
- If acid or alkali gets on the skin, it should be washed immediately with plenty of running water.
- If you light the spirit lamp immediately after removing the cap, a film of alcohol on the neck of the spirit lamp lights up just at the place where the cap is adjacent to the neck. The flame penetrates under the disk with the tube, and the alcohol vapor inside the tank ignites. There may be an explosion and ejection of the disc along with the wick. To avoid this, lift the disc with the wick for a few seconds to remove the vapors. If a fumes ignite, quickly put things aside (practical workbook) and call the teacher.
- Light the spirit lamp only with matches, extinguish with a lid or cap, covering from above.
- It is forbidden to transfer a lit spirit lamp and to light one spirit lamp from another.
- Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
- Experiments should be carried out with the amount of substances indicated in the methodological manual for each experiment.
- Without the permission of the teacher, do not touch anything on the tables.
- Maintain silence while conducting an experiment or writing a report.
- Clean up your workspace after work.
Page 184
What they were doing | Observations, drawings | Reaction equations | Conclusion |
Assemble the device. At the bottom of the test tube, place (with a pea) vaseline, copper oxide (II) (take 3 times more), mix. On the inside of the test tube, closer to the hole, use a spatula to place anhydrous copper (II) sulfate - powder white color. Pour the lime water solution into the receiving test tube and lower the gas outlet tube into it. Heat the entire tube first, then the bottom of the tube. Note signs of reactions taking place: a) with a mixture of vaseline and copper (II) oxide; b) with white powder of copper sulfate (II); c) with lime water. | figure ris3 a) Formation of a red coating on a mixture of vaseline and copper (II) oxide. b) White powder CuSO4 becomes blue. c) Lime water becomes cloudy. | WITH15 H32 + 46CuO →15CO2 + 16H2 O+46Cu CuSO4 +5N2 O → CuSO4 5N2 O CO2 + Ca(OH)2 → CaCO3 ↓+H2 O | . CuO is reduced to copper. CuO is an oxidizing agent, Vaseline is a reducing agent. When vaseline CuO is oxidized, water vapor is formed, which reacts with anhydrous CuSO4 . That. vaseline contains hydrogen. When Vaseline is oxidized with CuO, carbon dioxide is formed, which reacts with lime water. That. vaseline contains carbon. |
Conclusion:The composition of petroleum jelly includes carbon and hydrogen atoms, because. as a result of the oxidation of vaseline with copper (II) oxide, carbon dioxide and water are formed.
Practical work No. 6.
Solving experimental problems on the topic "Metals".
Target:study the properties of metals and their compounds.
Equipment and reagents:
Option 1: test tube rack, test tubes, iron, solutions of nitric acid, sulfuric acid, hydrochloric acid, sodium hydroxide, potassium chloride, potassium carbonate, copper (II) chloride, iron (II) chloride, nickel (II) sulfate,silver nitrate.
Option 2: test tube rack, test tubes, solutions of nitric and hydrochloric acid, iron (III) chloride, sodium hydroxide, potassium thiocyanate, sodium phosphate, zinc sulfate, sodium bromide,silver nitrate.
Progress:
Remember the safety rules when performing a chemical experiment.
- In a chemical laboratory, even known substances are not tasted, they may contain impurities that are toxic to humans.
- Acids are corrosive substances. Destroy and irritate the skin, mucous membranes.
- Alkalis are caustic substances. Destroy and irritate the skin, mucous membranes. They can cause complete loss of vision.
- If acid or alkali gets on the skin, it should be washed immediately with plenty of running water.
- Copper compounds in the form of dust upon contact with the skin, especially in places of microtrauma, can cause irritation, lead to mild allergies.
- All nitrates have a burning effect on the skin and mucous membranes. Silver nitrate (lapis) decomposes when exposed to sunlight. Causes darkening of the skin upon contact.
- The thiocyanates are compounds of increased physiological activity. When working with them, you should use personal protective equipment, observe the rules of personal hygiene.Do not allow drugs to enter the body!
- Glass is a brittle material with low impact resistance and low bending strength. It is strictly forbidden to use dishes that have cracks and broken edges.
- The test tube is fixed in the holder so that there is a distance of 1–1.5 cm from the neck of the test tube to the holder.
- Experiments should be carried out with the amount of substances indicated in the methodological manual for each experiment.
- Without the permission of the teacher, do not touch anything on the tables.
- Maintain silence while conducting an experiment or writing a report.
- Clean up your workspace after work.
Page 255
I option
Exercise 1.
Using the necessary reagents and equipment, perform the following transformations:
Fe → FeSO4 → Fe(OH)2 → Fe(NO3 ) 2
What they were doing | Observations | Reaction equations |
1. We put iron shavings in a solution of sulfuric acid. | Gas release. | Fe + H2 SO4 →FeSO4 + H2 Fe + 2Н+ →Fe2+ + H2 |
2. After a while, add a few drops of alkali to the resulting solution. | A greenish gelatinous precipitate forms. | FeSO4 + 2NaOH → Fe(OH)2 ↓ + Na2 SO4 Fe2+ + 2OH- → Fe(OH)2 ↓ |
3. | The precipitate dissolves.Reaction equations |
|
1. Add a few drops of alkali to a solution of nickel (II) sulfate. | A light green precipitate forms. | NiSO4 + 2NaOH → Ni(OH)2 ↓ + Na2 SO4 Ni2+ + 2OH- → Ni(OH)2 ↓ |
| The precipitate dissolves. | Ni(OH)2 + 2HCl → NiCl2 + 2H2 O Ni(OH)2 + 2H+ → Ni2+ + 2H2 O |
3. To anothertest tube to the resulting sediment add conc. alkali solution. | No changes. |
Conclusion:Nickel (II) hydroxide is a light green precipitate that exhibits basic properties.
Task 3.Suggest the most rational way to determine the salts, the solutions of which are in numbered test tubes: KCl, K2 CO3 , CuCl2 , FeCl2. ↓ blue gelatinous
Fe(OH)2 ↓ greenish gelatinous
HCl
no change
"boiling" CO2
AgNO3
AgCl↓
White
curdled
tube number:
CuCl2 + 2NaOH → Cu(OH)2 ↓ + 2NaCl
Cu2+ + 2OH- → Cu(OH)2 ↓
FeCl2 + 2NaOH → Fe(OH)2 ↓ + 2NaCl
Fe2+ + 2OH- → Fe(OH)2 ↓
K2 CO3 + 2HCl → 2KCl + CO2 + H2 O
2H+ + CO3 2- → CO2 + H2 O
KCl + AgNO3 → KNO3 + AgCl↓
Ag+ +Cl- → AgCl ↓
Conclusion:Substances can be identified using qualitative reactions.
II option:
Exercise 1.
Using the appropriate reagents and equipment, perform the following transformations
FeCl3 → Fe(OH)↓
2. Add a solution of nitric acid to the resulting precipitate.
The precipitate dissolves and a yellow solution is formed.
Fe(OH)3 + 3HNO3 → Fe(NO3 ) 3 + 3H2 O
Fe(OH)3 + 3H+ → Fe3+ + 3H2 O
3. Add a few drops of potassium thiocyanate to a solution of iron (III) nitrate.
The appearance of a blood-red color.
Fe(NO3 ) 3 + 3KCNS → Fe(CNS)3 + 3KNO3
Fe3+ + 3CNs- ↔ Fe(CNS)3
Conclusion:Experimentally carried out the transformation of chemical reactions.
Task 2.Prepare iron(III) hydroxide and investigate its properties.
What they were doing | Observations | Reaction equations |
1. Add a few drops of alkali to a solution of iron (III) chloride. | A brown precipitate forms. | FeCl3 + 3NaOH → Fe(OH)3 ↓ + 3NaCl Fe3+ + 3OH- → Fe(OH)3 ↓ |
2. The resulting sediment is divided into 2 parts. In oneadd a solution of hydrochloric acid to the resulting precipitate. | The precipitate dissolves. | Fe(OH)3 + 3HCl → FeCl3 + 3H2 O Fe(OH)3 + 3H+ → Fe3+ + 3H2 O |
3. To anothertest tube to the resulting sediment add conc. alkali solution, heat. | The precipitate dissolves. | t Fe(OH)3 + 3NaOH → Na3 Fe(OH)3 + 3OH- → 3- |
Conclusion:Iron hydroxide (III) - a brown precipitate, exhibits amphoteric properties.
Task 3.Suggest the most rational way to determine the salts, the solutions of which are in numbered test tubes: Na3 PO4
Fe(OH)3 ↓
brown
Zn(OH)2 ↓
White
no change
AgNO3
Ag3 PO4 ↓
yellow
AgBr↓
yellowish
curdled
tube number:
FeCl3 + 3NaOH → Fe(OH)3 ↓ + 3NaCl
Fe3+ + 3OH- → Fe(OH)3 ↓
ZnSO4 + 2NaOH → Zn(OH)2 ↓ + Na2 SO4
Zn2+ + 2OH- → Zn(OH)2 ↓
Na3 PO4 + 3AgNO3 → 3NaNO3 + Ag3 PO4 ↓
3Ag+ +PO4 3- → Ag3 PO4 ↓
NaBr + AgNO3 → NaNO3 + AgBr↓
Ag+ +Br- → AgBr ↓
Conclusion:Substances can be identified using qualitative reactions.
Practical work No. 1
Option number 1
Objective: Solution of experimental problems consisting of a chain of transformations.
Equipment: Rack with test tubes.
Reagents: Magnesium sulfate MgSO 4, alkali NaOH, barium chloride BaCl 2, sulfuric acid H 2 SO 4
MgSO 4 – MgCl 2 – Mg(OH) 2 - MgSO 4
| Reaction equations | Observations |
|
| MgSO4+ Mg 2+ + SO 4 2- + | ||
| MgCl 2 + Mg 2+ + 2Cl - + | ||
| Mg (OH) 2 + |
Conclusion:
Practical work No. 1
Implementation of a chain of chemical transformations of metals
Option 2
Safety briefing.
Purpose of work s: Solution of experimental problems consisting of a chain of transformations.
Equipment: Test tube rack, spirit lamp, matches, test tube holder
Reagents: Copper sulfate CuSO 4, alkali NaOH, sulfuric acid H 2 SO 4
CuSO 4 –Cu(OH) 2 – CuO – Cu SO 4
| Reaction equations | Observations |
|
| CuSO4+ | ||
| Cu (OH) 2 | ||
| CuO+ |
Conclusion:
"Practical work No. 2"
Practical work №2
Safety briefing.
Objective
Equipment: Rack with test tubes.
Reagents:
Option 1
Exercise 1.
| Reaction equations | Observations |
|
| AlCl 3 + NaOH = | ||
| NaOH + AlCl 3 = |
Conclusion:
Task 2
| Reaction equations | Observations |
|
| Al (OH) 3 + HCl \u003d | ||
| Al (OH) 3 + NaOH \u003d |
Conclusion:
Task3.
| Reaction equations | Observations |
|
| CaCl2+ | ||
| CaCl2+ |
Conclusion:
Practical work №2
Preparation and properties of metal compounds
Safety briefing.
Objective: Empirically prove the amphotericity of aluminum. .
Equipment: Rack with test tubes.
Reagents: AlCl 3 , NaOH , HCl , FeSO 4 , BaCl 2 , K 3 .
Option 2
Exercise 1. Determine whether the result of the reaction depends on the order in which the reactants are poured.
| Reaction equations | Observations |
|
| AlCl 3 + NaOH = | ||
| NaOH + AlCl 3 = |
Conclusion:
Task 2. Investigation of the properties obtained by Al (OH) 3 .
| Reaction equations | Observations |
|
| Al (OH) 3 + HCl \u003d | ||
| Al (OH) 3 + NaOH \u003d |
Conclusion:
Task3. Prove the qualitative composition of FeSO 4
| Reaction equations | Observations |
|
| FeSO 4 + K 3 \u003d | ||
| FeSO4 + |
Conclusion:
View document content
"Practical work No. 3"
Practical work No. 3
Safety briefing.
Objective
Equipment: rack with test tubes.
Reagents: NaOH , K 2 CO 3 , BaCl 2 , indicator paper, H 2 SO 4 , aluminum powder.
Option number 1
Progress
Task1 . Determine in which test tube each of the substances is located: NaOH, K 2 CO 3, BaCl 2.
Watching:…
Conclusion:
2. Let's determine the test tube in which the alkali is located with indicator paper:
Test tube No. 1 - color: ...
No. 2- color: ...
No. 3- color: ...
Conclusion: there is alkali in test tube No. ....
3. Pour in pr No. ... H 2 SO 4
(.).
Conclusion: in test tube No. … is……..
Task2. Get NaAlO 2 from Al .
1. Add an excess of alkali to a test tube with aluminum powder:
(Observation, reaction equations, conclusions.)
| What do I do? | What am I watching? | Reaction equations or deductions |
Practical work No. 3
Solving experimental problems for the recognition and production of substances
Safety briefing.
Objective: to learn by experience to determine and receive substances.
Equipment: rack with test tubes.
Reagents: Na 2 SO 4 , CaCO 3 , KCl , BaCl 2 , HCl , iron filings.
Option number 2
Progress
Task1 . Determine in which test tube each of the substances is located: Na 2 SO 4, CaCO 3, KCl.
1. Pour H 2 O into each test tube.
We observe the dissolution of substances: ...
Conclusion: in test tube No. … is ……..
2. Add HCl to the test tube:
(Observation, reaction equations.)
Conclusion: in test tube No. … is ……..
3. Pour in pr No. ... BaCl 2
(Observation, reaction equations, conclusions.)
Conclusion: in test tube No. … is ……..
Task2 . ReceiveFeCl 2 fromFe .
Add HCl to the test tube with iron filings:
(Observation, reaction equations, conclusions.)
Arrange the results in the form of a table:
| What do I do? | What am I watching? | Reaction equations or deductions |
View document content
"Practical work No. 4"
Practical work No. 4
Solving experimental problems on the topic "Oxygen subgroup"
Safety briefing.
Objective: to consolidate the theoretical knowledge of qualitative reactions in practice.
Equipment: rack with test tubes, cup for evaporation, spirit lamp.
Reagents: indicator phenolphthalein, AgNO 3 , BaCl 2 , NaOH , H 2 SO 4 , HCl , NaCl , KI , ZnSO 4 .
Progress
Exercise 1. Determine in which test tube each of the substances is located: NaOH, H 2 SO 4, HCl. (p. 147 No. 4).
Conclusion: test tube No. ... is located ... ..
Task2. Give qualitative reactions for substances: NaCl, KI, ZnSO 4 .(p. 147 No. 6).
Conclusion: high-quality reagents for ions ..... are ......
Task 3. Get from CuO , CuSO 4 , and CuSO 4 ∙5H 2 O . (p. 147 No. 7).
Conclusion:
Arrange the results in the form of a table:
| What do I do? | What am I watching? | Reaction equations or deductions |
View document content
"Practical work No. 5"
Practical work No. 5
Safety briefing.
Objective
Equipment: rack with test tubes.
Reagents: NH 4 Cl, NaOH, HCl, CaCO 3 , AgNO 3 , BaCl 2 , Na 2 SO 4 , K 2 CO 3 , Na 2 SiO 3
Option 1
Progress
Exercise 1. Prove empirically that the composition of ammonium chloride includes Cl - andNH 4 +
Conclusion:
Task 2 Na 2 SO 4 , K 2 CO 3 , Na 2 SiO 3 . Determine which substance is in each test tube. Give the reaction equations in molecular, full and reduced ionic form.
Conclusion:
Arrange the results in the form of a table:
| What do I do? | What am I watching? | Reaction equations or deductions |
Practical work No. 5
Solving experimental problems on the topic "Subgroup of nitrogen and carbon"
Safety briefing.
Objective: to learn by experience to determine the qualitative composition of the substance.
Equipment: rack with test tubes.
Reagents: NH 4 Cl, NaOH, HCl, CaCO 3 , AgNO 3 , BaCl 2 , ZnCl 2 , K 2 CO 3 , Na 2 SiO 3
Option 2.
Progress
Exercise 1. Prove empirically that the composition of ammonium sulfate includes SO 4 2- andNH 4 + ions. Give the reaction equations in molecular, full and reduced ionic form.
Conclusion:
Task 2. The test tubes contain crystalline substances: ZnCl 2 , K 2 CO 3 , Na 2 SiO 3 , Determine what substance is in each test tube Give the reaction equations in molecular, full and abbreviated ionic form.
Conclusion:
Arrange the results in the form of a table:
| What do I do? | What am I watching? | Reaction equations or deductions |
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"Practical work No. 6"
Practical work No. 6
Safety briefing.
Objective: to learn by experience how to receive, collect and recognize carbon dioxide
Equipment: stand with test tubes, splinter, matches
Reagents: HCl , CaCO 3 .
Option 1.
Progress
1. Conduct an experiment for obtaining CO 2
Observations:
2. Write a reaction equation for obtaining CO 2 in molecular, full and reduced ionic form.
4. Bring observations to the recognition of CO 2
| What do I do? | What am I watching? | Reaction Equations and Conclusions |
Conclusion:
Practical work No. 6
Receiving, collecting and recognizing gases
Safety briefing.
Objective: learn by experience to receive, collect and recognize hydrogen.
Equipment: stand with test tubes, matches.
Reagents: HCl, zinc
Option 2.
Progress
1. Conduct the experience of obtaining H 2
Observations
2. Compose a reaction equation, obtaining H 2 in molecular, full and reduced ionic form.
3. Characterize the reaction (reversibility, endo-exothermicity, compounds - decomposition, etc.)
4. Bring observations to recognize H 2
Arrange the result in the form of a table:
| What do I do? | What am I watching? | Reaction Equations and Conclusions |
Conclusion:
Practical work No. 6
Receiving, collecting and recognizing gases
Safety briefing.
Objective: to learn by experience to receive, collect and recognize oxygen.
Equipment: stand with test tubes, matches, splinter.
Reagents: KMpo 4
Option 3.
Progress
1. Conduct an experience of obtaining O 2
Observations
2. Write a reaction equation for obtaining O 2 in molecular, full and reduced ionic form.
3. Characterize the reaction (reversibility, endo-exothermicity, compounds - decomposition, etc.)
4. Bring observations to recognize O 2
Arrange the result in the form of a table:
| What do I do? | What am I watching? | Reaction Equations and Conclusions |
Conclusion:
View document content
"Practice 2 changed"
Practical work №2
Preparation and properties of metal compounds
Safety briefing.
Objective: Empirically prove the amphotericity of aluminum. Prove the qualitative composition of CaCO 3 .
Equipment: Rack with test tubes.
Reagents: AlCl 3 , NaOH , HCl , CaCL 2 , AgNO 3 , Na 2 CO 3
Option 1
Progress
Exercise 1. Determine whether the result of the reaction depends on the order in which the reactants are poured.
b) add AlCl 3 to NaOH
Task 2. Investigation of the properties obtained by Al (OH) 3 .
b) Al (OH) 3 + NaOH =
Task3. Prove the qualitative composition of CaCL 2
Conduct an experiment: a) CaCl 2 + ......
b) CaCl 2 + ……..
conclude, put the results in a table:
Practical work №2
Preparation and properties of metal compounds
Safety briefing.
Objective
Equipment: Rack with test tubes.
Reagents: AlCl 3 , NaOH , HCl , FeSO 4 , BaCl 2 , K 3 .
Option 2
Progress
Exercise 1. Determine whether the result of the reaction depends on the order in which the reactants are poured.
Conduct an experiment: a) add NaOH to AlCl 3
b) add AlCl 3 to NaOH
Make a conclusion, put the results in a table:
Task 2. Investigation of the properties obtained by Al (OH) 3 .
Conduct an experiment: a) Al (OH) 3 + HCl \u003d
b) Al (OH) 3 + NaOH =
conclude, put the results in a table:
Task3. Prove the qualitative composition of FeSO 4
Conduct an experiment: a) FeSO 4 + K 3 =
b) FeSO 4 + ……..
conclude, put the results in a table:
Draw a general conclusion about the work done.
