Practical work 1 chemistry 9. Instructions for performing practical work

Practical work No. 1

on this topic: "»

Purpose of work:

Equipment:

Progress

1. Tripod device

2.The device of the spirit lamp

3. Dishes

4.Filtering

3. put into the funnel;

"8th grade"

Practical work No. 1

on this topic: "Safety regulations when working in a chemical room. Techniques for handling laboratory equipment and heating devices»

Safety briefing.

Purpose of work: Become familiar with the device and basic techniques for handling laboratory equipment.

Equipment: Tripod, spirit lamp, laboratory glassware.

Progress

1. Tripod device(draw a tripod, mark its components)

2.The device of the spirit lamp(draw a spirit lamp, mark 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 to the center, so as not to splash out.

Find definitions of filtrate, cake and filtration process in the text.

Practical work No. 2

on this topic: « Observation of the changes occurring with a burning candle and their description»

Target: observe the physical and chemical phenomena when burning a candle.

Equipment: slide, candle, matches, dry test tube, holder.

Glass is a brittle material with low impact resistance and low flexural strength. It is strictly forbidden to use cookware with cracks and chipped 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 microscope slide is first heated completely, and then brought into the area of the dark cone of a burning candle.

First aid for burns:

First aid for cuts:

Experience number 1. Physical phenomena when burning a candle.

Light a candle. You will see how the paraffin wax 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 microscope slide, fix it in the holder ( t / b), bring into the area of the dark cone of a burning candle and hold for 3 - 5 s. Lift the glass quickly, look at the bottom plane. Explain what appeared there.

Secure the dry test tube in the holder ( t / b), turn upside down and hold over flame until fogging. Explain the observed phenomenon.

Practical work number 3

on this topic: "Soil and water analysis»

Target: determine the composition of the soil, learn how to filter and evaporate liquid.

Equipment: two test tubes, funnel, paper filter, glass rod, microscope slide, spirit lamp, glass cylinder with water, stopper, universal indicator paper.

Safety instructions:

The slide is neatly fixed in the holder at one of its edges. This takes into account that glass is a fragile material and can crack if you press hard on it.

In the process of evaporation of water from the soil extract, the entire glass slide is first warmed up, 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 closed 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, apply a sterile bandage after cooling the burn site and go to the first-aid post.

Experience number 1. Mechanical analysis of the soil.

Soil is placed in the test tube. Pour water to it, the volume of which should be 3 times the volume of the soil. Close the tube with a stopper and shake well for 1 - 2 minutes. Observe the sediment of the soil particles and the structure of the sediment. 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. Do not shake the mixture before filtering. The soil will remain on the filter, and the filtrate collected in the test tube is a soil extract (soil solution).

Using a glass rod, place a few drops of this solution 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 test paper, apply the soil solution to it with a glass stick. Draw a conclusion based on the results of your observations.

Practical work number 4

on this topic: "Preparation of sugar solution and determination of its mass fraction in solution»

Safety briefing

Target: learn to weigh on a laboratory balance, determine the volume of a liquid using a graduated cylinder, prepare a solution with a certain mass fraction of a substance.

Equipment and reagents: beaker, stirring rod, graduated cylinder, laboratory balance, 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)
Provide calculations in the report on practical work.

Determine the volume of water corresponding to the calculated mass using the formula: V =m · ρ. Remember that ρ = 1 g / ml for water.
The calculation is given in the report on practical work.

Use a graduated cylinder to measure out the calculated volume of water. Pour water into a beaker.

Weigh the calculated sugar mass on a laboratory scale. Pour sugar in a glass of water.

Stir the contents of the beaker until the sugar is completely dissolved.

Make a conclusion about what is necessary to prepare a solution with a certain mass fraction of a solute.

Practical work number 5

on this topic: "Signs of chemical reactions»

Target: consider examples of chemical reactions and identify their signs.

Equipment: test tubes, copper wire, alcohol 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 exactly where the cap adjoins the neck. The flame penetrates under the tube disc and the alcohol vapors inside the reservoir ignite. Explosion and ejection of the disc along with the wick may occur. To avoid this, lift the disc with the vapor wick for a few seconds. If the vapors ignite, quickly set aside the objects (practice notebook) and call the teacher.

A lighted spirit lamp should not be carried from place to place, nor should one spirit lamp be lit directly from another. Use matches to light the 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 so that when the bottle is tilted, the label is on top to avoid damage to it.

Copper compounds in the form of dust when in contact with the skin, especially in places of microtrauma, can cause irritation and lead to mild allergies.

Barium compounds must be handled in such a way as to avoid getting them into the mouth, as they are toxic. To obtain severe poisoning, a dose of less than 0.5 g is sufficient. After completing the 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);

c) after treatment, the wound is closed 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:

First aid in case of contact of acid on the skin of the hands:

Shake off drops of acid 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 Annealing of copper wire.

Light the spirit 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?

Experience No. 2 The interaction of sodium carbonate with hydrochloric acid.

Place some sodium carbonate in a small beaker. Pour enough hydrochloric acid into a beaker to cover the sodium carbonate. What are you watching?

Light the torch and place it in the glass. What are you watching?

Prepare your report by filling in the table.

Experience No. 3 The interaction of ammonium chloride with sodium hydroxide.

Put some ammonium chloride in a test tube. Pour enough sodium hydroxide solution into the test tube to cover the ammonium chloride. Shake well. Sniff the contents of the tube gently.

Prepare your report by filling in the table.

Experience No. 4 The 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?

Prepare your report by filling in the table.

Experience No. 5 The interaction of copper hydroxide ( II ) with hydrochloric acid.

Pour a little hydrochloric acid solution to copper (II) hydroxide. Shake gently. What are you watching?

Prepare your report by filling in the table.

Experience No. 6 Combustion of alcohol

Pour 2 ml of ethanol into a cup. Light it on fire. What are you watching? Prepare your report by filling in the table.

Experiment No. 7 Decomposition of malachite

Pour a small amount of malachite into a test tube. Heat it up in a spirit lamp flame. What are you watching?

Prepare your report by filling in the table.

What they were doing	Observations	(sign of a chemical reaction)

Practical work number 6

on this topic: "Properties of acids, bases, oxides and salts»

Target: to carry out in practice the reactions characterizing the properties of acids, bases, oxides and salts.

Equipment and reagents: a 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
Test 1




Test 2

Work order

Experience 1. Carry out the reactions characterizing the properties of the sulfuric acid solution:

a) acid + metal = salt + H 2

b) acid + basic oxide = salt + H 2 O

c) acid + base = salt + H 2 O

d) acid + salt = salt + acid

Test 2... Perform the reactions characterizing the properties of copper (II) chloride:

a) salt + metal = salt + metal

b) salt + alkali = base ↓ + salt

c) salt + acid = salt + acid

d) salt + salt = salt + salt ↓

Draw up the equations of the reactions performed in molecular and ionic form.

Practical work number 7

on this topic: "Experimental problem solving»

Target: experimentally carry out the tasks.

Equipment and reagents: a 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 diagrams of which are given:

a) Ba 2+ + SO 4 2- = BaSO 4

b) CO 3 2- + 2H + = H 2 O + CO 2

c) OH - + H + = H 2 O

In the table, write down observations and reaction equations in molecular full and abbreviated and ionic form.

Experience 2. Using the solutions on the table, you will get:

a) copper (II) hydroxide

b) magnesium carbonate

Write down the observations in the table. Write the reaction equations in molecular, full and abbreviated ionic form.

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"Grade 9"

Practical work No. 1

on this topic: "Implementation of a chain of chemical transformations»

Safety briefing.

purpose of work: Solving experimental problems consisting of a chain of transformations.

Equipment: Test tube rack.

Reagents (1c.): Magnesium sulfate MgSO 4, alkali NaOH, barium chloride BaCl 2.

Reagents (2c.): 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
	MgSO 4 + Mg 2+ + SO 4 2- +
	MgCl 2 + Mg 2+ + 2Cl - +
	Mg (OH) 2 +

Output:

Option 2: CuSO 4 –Cu (OH) 2 - CuO - Cu

	Reaction equations
	CuSO 4 +
	Cu (OH) 2
	CuO +

Output:

Practical work number 2

This appendix contains instructions for practical work for students in grade 9.

"Practical work No. 1 - 9 cells"

Practical work No. 1

purpose of work: Experimentally prove the amphotericity of aluminum. Prove the qualitative composition of CaCO 3.

Equipment: Test tube rack.

Reagents:

Option 1

Exercise 1.

	Reaction equations	Observations
	AlCl 3 + NaOH =
	NaOH + AlCl 3 =

Output:

Assignment 2

	Reaction equations
	Al (OH) 3 + НCl =
	Al (OH) 3 + NaOH =

Output:

Assignment 3. Prove the quality composition of CaCL 2

	Reaction equations
	CaCL 2 +
	CaCL 2 +

Output:

Practical work No. 1

Obtaining metal compounds and studying their properties

Safety briefing.

purpose of work: Experimentally prove the amphotericity of aluminum. Prove the quality composition of FeSO 4.

Equipment: Test tube rack.

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 reagents are merged.

	Reaction equations
	AlCl 3 + NaOH =
	NaOH + AlCl 3 =

Output:

Assignment 2... Investigation of properties obtained by Al (OH) 3.

	Reaction equations
	Al (OH) 3 + НCl =
	Al (OH) 3 + NaOH =

Output:

Assignment 3. Prove the quality composition of FeSO 4

	Reaction equations
	FeSO 4 + K 3 =
	FeSO 4 +

Output:

View document content
"Practical work No. 2 - 9 cells"

Practical work No. 2

Safety briefing.

purpose of work: Solving experimental problems consisting of a chain of transformations.

Equipment: Test tube rack.

Reagents

Option 1: MgSO 4 - MgCl 2 - Mg (OH) 2 - MgSO 4

	Reaction equations
	MgSO 4 + Mg 2+ + SO 4 2- +
	MgCl 2 + Mg 2+ + 2Cl - +
	Mg (OH) 2 +

Output:

Practical work No. 2

Implementation of a chain of chemical transformations of metals

Safety briefing.

Purpose of work s: Solving experimental problems consisting of a chain of transformations.

Equipment: Test tube rack.

Reagents: Copper sulfate CuSO 4, alkali NaOH, hydrochloric acid HCl, Fe (paper clip).

Option 2: CuSO 4 –Cu (OH) 2 - CuO - Cu

	Reaction equations
	CuSO 4 +
	Cu (OH) 2
	CuO +

Output:

View document content
"Practical work No. 3 - 9 cells"

Practical work No. 3

Safety briefing.

purpose of work

Equipment:

Reagents

Progress

Exercise 1.

Task 2. 4 .

Task 3.

Practical work No. 3

Solving experimental problems on the topic "Oxygen subgroup"

Safety briefing.

purpose of work: To consolidate theoretical knowledge of qualitative reactions in practice.

Equipment: Test tube rack, evaporation dish, 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.

Task 2. Lead qualitative reactions for substances NaCl, KI, ZnSO 4 .

Task 3. Get from CuO, Cu SO 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 of its properties.

Purpose of work: _________________________________________________________________

_____________________________________________________________________

Equipment: ________________________________________________________________

Reagents:

Name	Chemical formula

Hydrochloric acid
Lime water
Sodium carbonate

Precautionary measures: _____________________________________________________________

_____________________________________________________________________________________

Progress: Present the results of work in the form of a table

Experience name	What they were doing?	What did you observe?	Chemical reaction equation (in molecular, complete, 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 hydrocarbons			CO 2 + Ca (OH) 2 = CaCO 3 + CO 2 + H 2 O ↔ Ca (HCO 3) 2 t˚C →
Experience number 3. Recognition of carbonates			Na 2 CO 3 + HCl =

Output (fill the gaps):

Carbon monoxide (IV) in the laboratory can be obtained ________________________________________

_____________________________________________________________________________________

The following properties of CO 2 were 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 _______________ with the formation of ______________________.

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)

Theme:"Obtaining ammonia and studying its properties"

Purpose: Obtain ammonia and familiarize yourself with the properties of an aqueous solution of ammonia.

Equipment and reagents:

Instructions for the implementation of practical work.

Repeat the questions in the textbook: obtaining and properties of ammonia, ammonia water and ammonium salts. Then get to work.

Experience number 1. Ammonia production .

Assemble the ammonia generator.

Place four spatulas of ammonium chloride and two spatulas of calcium hydroxide in a porcelain bowl. 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 tripod leg (pay attention to the inclination of the test tube with the mixture). Put a dry test tube for collecting ammonia on the gas outlet tube and close its hole with a cotton swab.

Warm the test tube with a mixture of ammonium chloride and calcium hydroxide slightly (2-3 strokes of the flame), and then heat in the place where the mixture is located. To detect ammonia, bring a damp phenolphthalein paper to the opening of an upside-down test tube. Having found ammonia, bring a glass rod moistened with hydrochloric acid solution to the opening of the test tube. What are you watching? What is the chemical composition of the resulting particulate matter (smoke)? Write the reaction equation.

Stop heating the mixture. Carefully remove the tube containing ammonia from the gas outlet tube, holding it upside down (close the end of the gas outlet tube with a piece of wet cotton wool immediately after removing the ammonia tube from it).

Immediately close the opening of the removed tube with your thumb and place it in a container of water. Take your finger off 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 should a test tube with a mixture of substances for the production of ammonia be fixed in the tripod leg obliquely with a raised bottom?

2. Why is ammonia collected in an upside-down test tube? What other gases can be collected in this way?

3. How can you prove that an aqueous solution of ammonia contains hydroxide ions?

Perform the following experiments with the obtained aqueous ammonia solution.

Study of the properties of an aqueous solution of ammonia

Experience number 1. Pour 2-3 ml of an aqueous solution of ammonia 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 aqueous ammonia solution into a test tube. Add 2-3 drops of phenolphthalein and add sulfuric acid solution drop by drop until the raspberry color disappears. Why did the color disappear? Write the ionic reaction equations.

Draw up a work report. Make a conclusion.

The name of the experiment.	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
	Obtaining metal compounds and studying their properties	Equipment: Test tube rack. Reagents: AlCl 3, NaOH, HCl, CaCL 2, AgNO 3.
	Implementation of a chain of chemical transformations of metals	Equipment: Test tube rack. Reagents: Magnesium sulfate MgSO 4, alkali NaOH, barium chloride BaCl 2.
	Oxygen subgroup	Equipment: Test tube rack, evaporation dish, 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: alcohol lamp, metal stand, stopper with gas 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 gas outlet tube Reagents: marble, hydrochloric acid, lime water, sodium carbonate

Practical work No. 1.

The 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, alcohol lamp, holder, test tube rack, 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:

EXPERIENCE 1. Influence of the nature of the reacting substances.

EXPERIENCE 2. Influence of the concentration of reactants.

EXPERIENCE 3. Influence of the contact area of the reacting substances.

EXPERIENCE 4. Influence of temperature.

Put a little black powder of copper (II) oxide in de test tubes, add a solution of sulfuric acid to both test tubes. Heat one of the tubes

EXPERIENCE 5. Influence of the catalyst.

2 O 2 2 ... In which test tube does the reaction go faster? Why?

Draw up the work in the form of a table:

The considered factor affecting the rate of chemical. reactions	Description of the experiment	Observations to judge the reaction rate	Reaction equations	Output
Experience 1. Influence of the nature of the reacting substances.	Pour 2 ml of hydrochloric acid solution into three 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. Observe the speed of the three reactions. Which reaction is the fastest and why?	Gas evolution occurs most violently in a test tube containing 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 most powerful reducing properties.
Experience 2. Influence of the concentration of reactants.	In two test tubes, tilting them, lower them over the zinc granule, carefully pour the solutions of sulfuric acid: in the first test tube the acid solution is 1: 5, in the second - 1:10. In which of them does the reaction go faster?	In the first test tube, the gas is released more intensively.	Zn + H 2 SO 4 → ZnSO 4 + H 2	The higher the concentration of the reacting substances, the more often the collisions of their particles and the higher the rate of the chemical reaction.
Experience 3. Influence of the contact area of the reactants.	Pour a little iron powder into one tube, put an iron clip into the other and add 2 ml of diluted hydrochloric acid (1: 2) to both tubes.In which test tube does the reaction go faster? Why?	Gas evolution proceeds faster in a test tube with iron powder.	Fe + 2HCl → FeCl 2 + H 2	The larger the contact area of the reacting substances, the higher the rate of the chemical reaction.
Experience 4. Influence of temperature.	Put a little black powder of copper (II) oxide into two tubes, add a solution of sulfuric acid to both tubes. Heat one of the tubes. In which test tube does the reaction go faster? Why?	The dissolution of copper (II) oxide 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 movement of particles and the speed of the chemical reaction increase.
Experience 5. Effect 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 tubes 2 ... In which test tube does the reaction go faster? Why?	In the presence of manganese (IV) oxide, gas bubbles are vigorously evolved.	2H 2 O 2 2H 2 O + O 2	Manganese (IV) oxide is a catalyst that accelerates the decomposition reaction of hydrogen peroxide.

Output: The rate of a chemical reaction depends on the conditions: on the nature of the reacting substances, on the contact area, on concentration, on temperature, on the presence of catalysts.

Practical work No. 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 precautions 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 hold 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, rinse it immediately with plenty of running water.
Glass is a brittle material with low impact resistance and low flexural strength. It is strictly forbidden to use cookware with cracks and chipped edges.
Experiments should be carried out with such a number of substances, which are indicated in the methodological manual for each experiment.
Do not touch anything on the tables without the teacher's permission.
Be quiet when conducting an experiment or writing a report.
After work, clean up your workplace.

Task number 1. Determine empirically the composition of solutions without labels: sulfuric acid, sodium chloride, sodium sulfate.

Substance reagent	H 2 SO 4	NaCl	Na 2 SO 4
litmus	Red color	no change	no change
BaCl 2		no change	BaSO 4 ↓ White
AgNO 3		AgCl ↓ white cheesy
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.

Qualitative reaction for chloride anion - interaction with silver nitrate, a white curdled precipitate is formed.

НCl + AgNO 3 → НNO 3 + AgCl ↓

Ag + + Cl - → AgCl ↓

2) Copper (II) sulfate.

Copper (II) sulfate dissociates into ions: CuSO 4 → Cu 2+ + SO 4 2-

Qualitative reaction for sulfate ion is interaction with barium chloride. A white precipitate of barium sulfate forms:

CuSO 4 + BaCl 2 → CuCl 2 + BaSO 4 ↓

Ba 2+ + SO 4 2- → BaSO 4 ↓

Qualitative reaction for 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 ↓

Output:

Practical work No. 3.

Obtaining ammonia and studying its properties. Acquaintance with the chemical properties of an aqueous solution of ammonia.

Target: 1. To consolidate the ability to receive gases and collect them, taking into account the relative density of the air.

2. Study the properties of ammonia and ammonia water, learn to receive and recognize ammonium salts.

Equipment and reagents:laboratory stand, alcohol lamp, stopper with gas outlet 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 precautions 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 hold 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 corrosive substances. Destroy and irritate the skin, mucous membranes. From them, a complete loss of vision is possible.
If acid or alkali gets on the skin, rinse it immediately with plenty of running water.
Ammonia requires careful handling due to physiological activity and damages the respiratory tract (dehydration).Ammonia, which will be released during the interaction of ammonium salts with alkalis, is very soluble in water, and therefore in the moisture of the mucous membrane of the eyes. Their irritation may ensue. If this happens, rinse your 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 exactly where the cap adjoins the neck. The flame penetrates under the tube disc and the alcohol vapors inside the reservoir ignite. Explosion and ejection of the disc along with the wick may occur. To avoid this, lift the disc with the wick to remove the vapor for a few seconds. If the vapors ignite, quickly set aside the objects (practice notebook) 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 lighted spirit lamp and light one spirit lamp from another.
When heating a substance in a test tube, it must first be warmed up; the opening of the test tube during heating should be directed away from yourself and the neighbor.
Glass is a brittle material with low impact resistance and low flexural strength. It is strictly forbidden to use cookware with cracks and chipped edges.
Experiments should be carried out with such a number of substances, which are indicated in the methodological manual for each experiment.
Do not touch anything on the tables without the teacher's permission.
Be quiet when conducting an experiment or writing a report.
After work, clean up your workplace.

P. 116-117

Experience name	What they were doing	Observations, drawings	Reaction equations	Output
Experience 1. Getting ammonia and dissolving it in water.	In a porcelain mortar, stir equal volumes of solid ammonium chloride NH 4 Cl and calcium hydroxide Ca (OH) 2 ... Pour the prepared mixture into a test tube for 1/3 of its volume. Close the tube with a stopper with a gas outlet tube. Secure the tube at an angle so that the bottom is slightly higher than the stopper. Explain why? Place a dry test tube on the end of the gas outlet tube, covering the bottom of the hole with a cotton swab. Heat the mixture: first the whole tube, then the reaction mixture. Why is ammonia collected in an upside-down test tube? When you smell ammonia, plug the test tube with your finger and, without inverting, immerse it in a crystallizer with water. What are you seeing? What caused this phenomenon? Invert the tube with the solution, test with phenolphthalein. What are you seeing? Make a conclusion.	picture ris1.jpg Water vapor condenses at the plug. There is a smell of ammonia. Rapid suction of water into a test tube. The appearance of a raspberry color.	Ca (OH) 2 + 2NH 4 C1 CaCl 2 + 2NH 3 + 2H 2 O NH 3 + H 2 O ⇄ NH 3 H 2 O ⇄ NH 4 + + OH -	The neck of the tube is tilted slightly downward to prevent water droplets from dripping onto the warmer sides of the 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. Interaction of ammonia with acids.	Dip the gas outlet tube into ¼ test tubes filled with solutions of hydrochloric acid with sulfuric acid. What are you seeing?	Above the surface of acid solutions appears "white smoke" - crystalline ammonium chloride and sulfate.	NH 3 + HCl → NH 4 Cl NH 3 + H 2 SO 4 → (NH 4) 2 SO 4	Ammonia reacts actively with acids.
Experience 3. Interaction of ammonium salts with alkalis (recognition of ammonium salts)	Put a little crystalline ammonium sulfate in a test tube, add 2 ml of sodium hydroxide solution, heat slightly. How do you feel? Bring wet litmus paper to the opening of the test tube. What are you seeing? Draw a conclusion on how to recognize ammonium salts.	Gas is emitted with a pungent odor. It 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.

Output: We studied the properties of ammonia, learn how to receive and recognize ammonium salts.

Practical work No. 4.

Obtaining carbon monoxide (IV) and studying its properties. Recognition of carbonates.

Target: 1. Consolidate knowledge about the properties of carbon dioxide and carbonates.

2. Learn to receive carbon dioxide by exchange reaction and recognize it.

Equipment and reagents:laboratory tripod, stopper with gas tube, 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 precautions 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, rinse it immediately with plenty of running water.
Barium compounds must be handled in such a way as to avoid getting them into the mouth, as they are toxic. To obtain severe poisoning, a dose of less than 0.5 g is sufficient. After completing the work, wash your hands thoroughly with soap and running water.

Glass is a brittle material with low impact resistance and low flexural strength. It is strictly forbidden to use cookware with cracks and chipped 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 such a number of substances, which are indicated in the methodological manual for each experiment.
Do not touch anything on the tables without the teacher's permission.
Be quiet when conducting an experiment or writing a report.
After work, clean up your workplace.

Test 1 ... Obtaining carbon monoxide (IV) and studying its properties. P. 158-159

What they were doing

Observations, drawings

Reaction equations

Output

Assemble the gas generating device. Check it for leaks. Place a few pieces of marble in a test tube and add 2 ml dil. of hydrochloric acid.

What are you seeing?

Close the tube with a stopper with a gas outlet tube and pass the evolved gas through lime water. What do you watching?

Continue passing gas for a few minutes. What are you seeing?

Place the end of the gas outlet tube into a test tube with 2-3 ml of distilled water and a few drops of litmus and pass carbon dioxide gas through it. What are you seeing?

figure ris2

Violent gas evolution.

Turbidity of lime water.

The resulting precipitate dissolves.

Litmus turns red.

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, to obtain carbon dioxide, carbonates are acted upon with a strong acid.

Lime water is used to detect carbon dioxide.

With an excess of carbon dioxide, insoluble carbonates transform into soluble bicarbonates.

When carbon dioxide dissolves, carbonic acid is formed. 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.

Test 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	Na 2 SO 4	Na 2 CO 3
	no change	no change	"Boiling" CO 2
BaCl 2	no change	BaSO 4 ↓ White
AgNO 3	AgCl ↓ white cheesy
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 ↓

Output:1. It is possible to recognize substances using qualitative reactions.

2. Qualitative reaction to carbonate ion - interaction of carbonates with strong acids.

Practical work No. 5.

Determination of the qualitative composition of organic matter.

Target:learn to empirically determine the qualitative composition of organic substances.

Equipment and reagents:laboratory stand, spirit lamp, stopper with gas outlet tube, test tubes, anhydrous copper (II) sulfate, copper (II) oxide, petroleum jelly, lime water.

Progress:

Remember the safety precautions when performing a chemical experiment.

Alkalis are corrosive substances. Destroy and irritate the skin, mucous membranes. From them, a complete loss of vision is possible.
If acid or alkali gets on the skin, rinse it 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 exactly where the cap adjoins the neck. The flame penetrates under the tube disc and the alcohol vapors inside the reservoir ignite. Explosion and ejection of the disc along with the wick may occur. To avoid this, lift the disc with the wick to remove the vapor for a few seconds. If the vapors ignite, quickly set aside the objects (practice notebook) 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 lighted spirit lamp and light one spirit lamp from another.
Glass is a brittle material with low impact resistance and low flexural strength. It is strictly forbidden to use cookware with cracks and chipped edges.
Experiments should be carried out with such a number of substances, which are indicated in the methodological manual for each experiment.
Do not touch anything on the tables without the teacher's permission.
Be quiet when conducting an experiment or writing a report.
After work, clean up your workplace.

P. 184

What they were doing

Observations, drawings

Reaction equations

Output

Assemble the device.

At the bottom of the test tube, place (about a pea) petroleum jelly, copper (II) oxide (take 3 times more), mix. On the inside of the tube, close to the hole, place anhydrous copper (II) sulfate - white powder with a spatula. Pour lime water solution into the receiving tube and lower the gas outlet tube into it. Warm up the whole tube first, then the bottom of the tube.

Note the signs of reactions that are occurring:

a) with a mixture of petroleum jelly and copper (II) oxide;

b) with white powder of copper (II) sulfate;

c) with lime water.

figure ris3

a) Formation of red plaque on a mixture of petroleum jelly and copper (II) oxide.

b) White powder CuSO4 becomes blue.

c) Lime water becomes cloudy.

WITH15 H32 + 46CuO → 15CO2 + 16H2 O + 46Cu

CuSO4 + 5H2 O → CuSO4 5H2 O

CO2 + Ca (OH)2 → CaCO3 ↓ + H2 O

Reduction of CuO to copper occurs. CuO is an oxidizing agent, petroleum jelly is a reducing agent.

The oxidation of petrolatum CuO produces water vapor, which reacts with anhydrous CuSO4 ... That. petrolatum contains hydrogen.

The oxidation of Vaseline CuO produces carbon dioxide, which reacts with lime water. That. petrolatum contains carbon.

Output:Vaseline contains carbon and hydrogen atoms. as a result of the oxidation of petroleum jelly 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: a rack for test tubes, 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: a rack for test tubes, 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 precautions 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 corrosive substances. Destroy and irritate the skin, mucous membranes. From them, a complete loss of vision is possible.
If acid or alkali gets on the skin, rinse it immediately with plenty of running water.
Copper compounds in the form of dust when in contact with the skin, especially in places of microtrauma, can cause irritation and 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 skin darkening on contact.
Rodanides are compounds with 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 flexural strength. It is strictly forbidden to use cookware with cracks and chipped 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 such a number of substances, which are indicated in the methodological manual for each experiment.
Do not touch anything on the tables without the teacher's permission.
Be quiet when conducting an experiment or writing a report.
After work, clean up your workplace.

P. 255

Option I

Exercise 1.

Using the necessary reagents and equipment, carry out 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 evolution.	Fe + H2 SO4 → FeSO4 + H2 Fe + 2H+ → Fe2+ + H2
2. After a while, add a few drops of alkali to the resulting solution.	A greenish gelatinous precipitate is formed.	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 the nickel (II) sulfate solution.	A light green precipitate is formed.	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 anotheradd a test tube to the resulting sediment with conc. alkali solution.	No changes.

Output:Nickel (II) hydroxide is a light green precipitate that exhibits basic properties.

Task 3.Suggest the most rational way to determine salts, solutions of which are in numbered test tubes: KCl, K2 CO3 , CuCl2 , FeCl2. ↓ blue gelatinous

Fe (OH)2 ↓ greenish gelatinous

HCl

no change

"Boiling" of CO2

AgNO3

AgCl ↓

White

cheesy

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 ↓

Output:Substances can be recognized using qualitative reactions.

Option II:

Exercise 1.

Using the necessary reagents and equipment, carry out the following transformations

FeCl3 → Fe (OH)↓

2. Add a nitric acid solution to the resulting precipitate.

The precipitate dissolves, 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 the solution of iron (III) nitrate.

The appearance of a blood red coloration.

Fe (NO3 ) 3 + 3KCNS → Fe (CNS)3 + 3KNO3

Fe3+ + 3CNS- ↔ Fe (CNS)3

Output:Experimentally carried out the transformation of chemical reactions.

Task 2.Prepare iron (III) hydroxide and research its properties.

What they were doing	Observations	Reaction equations
1. Add a few drops of alkali to the solution of iron (III) chloride.	A brown precipitate is formed.	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 sediment.	The precipitate dissolves.	Fe (OH)3 + 3HCl → FeCl3 + 3H2 O Fe (OH)3 + 3H+ → Fe3+ + 3H2 O
3. To anotheradd a test tube to the resulting sediment with conc. alkali solution, heat.	The precipitate dissolves.	t Fe (OH)3 + 3NaOH → Na3 Fe (OH)3 + 3OH- → 3-

Output:Iron (III) hydroxide is a brown precipitate that exhibits amphoteric properties.

Task 3.Suggest the most rational way to determine salts, 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

cheesy

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 ↓

Output:Substances can be recognized using qualitative reactions.

Grade 9. Practical work No. 1. OBTAINING AMPHOTHERIC HYDROXIDE AND RESEARCH OF ITS PROPERTIES. Progress. A) Perform experiments and formalize the work. EXPERIENCE 1. Obtaining aluminum hydroxide. Pour a small amount of aluminum chloride into a test tube and add sodium hydroxide dropwise to it. What are you watching? Put the results of the experiment in a table. Do the experiment three times. Figure of the experiment Equations of reactions Conclusions EXPERIMENT 2. Interaction with acids. Gently add a solution of nitric acid to aluminum hydroxide. What are you watching? Put the results of the experiment in a table. Figure of the experiment Equations of reactions Conclusions EXPERIMENT 3. Interaction with alkalis. Gently add sodium hydroxide to aluminum hydroxide. What are you watching? Put the results of the experiment in a table. Figure of the experiment Equations of reactions Conclusions EXPERIMENT 4. Decomposition of insoluble hydroxides. Warm up the aluminum hydroxide tube gently. What are you watching? Put the results of the experiment in a table. Drawing of experiment Equations of reactions Conclusions B) Make a final conclusion on the whole work. C) Remove the workplace.

Grade 9. Practical work No. 1. OBTAINING AMPHOTHERIC HYDROXIDE AND RESEARCH OF ITS PROPERTIES. REACTIONS AND ABOUT BORUDO VAN AND E. 3 test tubes, asbestos mesh, cap, matches, rubbish glass, fuel, test tube holder, AlCl3, NaOH, HNO3.

Grade 9. Practical work No. 2. RECOGNITION OF METAL CATIONS. Progress. A) Perform experiments and formalize the work. EXPERIENCE 1. Recognition of Na + Heat the crystalline salt of sodium chloride on a copper wire in a burner flame. What are you watching? Put the results of the experiment in a table. Figure of the experiment Reaction equations 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? Put the results of the experiment in a table. Figure of experiment Equations of reactions 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? Put the results of the experiment in a table. Figure of experiment Equations of reactions 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? Put the results of the experiment in a table. Figure of experiment 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 dropwise to it. What are you watching? Put the results of the experiment in a table. Figure of experiment Equations of reactions Conclusions EXPERIMENT 6. Recognition of Fe2 + Pour a solution of iron (II) chloride into a test tube and add a solution of sodium hydroxide to it. What are you watching? Put the results of the experiment in a table. Drawing of experiment Equations of reactions Conclusions EXPERIMENT 7. Recognition of Fe3 +

Pour iron (III) chloride solution into a test tube and add sodium hydroxide solution to it. What are you watching? Put the results of the experiment in a table. Drawing of experiment Equations of reactions Conclusions B) Make a final conclusion on the whole work. C) Remove the workplace. Grade 9. Practical work No. 2. RECOGNITION OF METAL CATIONS. R E A C T I S AND ABOUT B O R D O V A N I E. 6 test tubes, copper wire, asbestos mesh, fuel, cap, matches, rubbish glass, test tube holder, NaCl (crystal), CaCl2 , Na2CO3, BaCl2, H2SO4, AgNO3, HCl, AlCl3, NaOH, FeCl2, FeCl3.

Grade 9. Practical work No. 3. PRACTICAL IMPLEMENTATION OF CHAINS OF TRANSFORMATION. Option 1. 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. Option 3. 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. Option 4. 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 ANION. Progress. A) Perform experiments and formalize the work. EXPERIMENT 1. Recognition of Cl Add a small amount of silver nitrate to the sodium chloride solution. What are you watching? Put the results of the experiment in a table. Figure of the experiment 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? Put the results of the experiment in a table. 2 Figure of the experiment Equations of reactions Conclusions EXPERIMENT 3. Recognition of СО3 Pour a solution of sodium carbonate into a test tube and add a solution of sulfuric acid to it. What are you watching? Put the results of the experiment in a table. 2 Figure of experiment Reaction equations Conclusions EXPERIMENT 4. Recognition of PO4 Pour sodium phosphate solution into a test tube and add a drop of silver nitrate to it. What are you watching? Put the results of the experiment in a table. 3 Figure of experiment Reaction equations Conclusions EXPERIMENT 5. Recognition of SiO3 Pour sodium silicate solution into a test tube and add sulfuric acid solution dropwise to it .. What do you observe? Put the results of the experiment in a table. 2

Figure of the experiment Reaction equations 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? Put 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? Put the results of the experiment in a table. Figure of experiment 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. Warm up the tube gently. What are you watching? Put the results of the experiment in a table. Figure of experiment Reaction equations Conclusions EXPERIMENT 9. Recognition of S2 Pour sodium sulfide solution into a test tube and add sulfuric acid solution to it. What are you watching? Put the results of the experiment in a table. Figure of the experiment Reaction equations Conclusions EXPERIMENT 10. Recognition of OH Drop a drop of sodium hydroxide on the indicator paper. What are you watching? Put the results of the experiment in a table. Drawing of experiment Equations of reactions Conclusions B) Make a final conclusion for the whole work. C) Remove the workplace.

Grade 9. Practical work No. 8. RECOGNITION OF THE MOST IMPORTANT ANION. R E A C T I S AND ABOUT W A N I E. 9 test tubes, indicator paper, glass of water, glass rod, asbestos mesh, fuel, matches, glass for rubbish, 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. Get copper (II) nitrate in two different ways. Write down the reaction equations in molecular and ionic forms. Record the results of the experiments in the table. Figure of the experiment Reaction equations Conclusions Experiment 2. Prove the qualitative composition of acids: Option 1: hydrochloric acid Option 2: sulfuric acid Option 3: phosphoric acid. Write down the reaction equations in molecular and ionic forms. Put the results of the experiment in a table.

Drawing of experiment Equations of reactions Conclusions Experiment 3. Practical way to carry out a chain of transformations: Mg Write down the equations of reactions in molecular and ionic forms. Record the results of the experiments in the table. Mg (OH) MgCl Mg (NO 3) 2 → 2 → → 2 Figure of the experiment Equations of reactions Conclusions  Make a final conclusion on the work.  Clean up the workplace. Grade 9. Practical work No. 9. SOLUTION OF EXPERIMENTAL PROBLEMS. ABOUT R U D O V A N E I R E A K T I V S. 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.

Material description: Presents the development of the entire practical course in chemistry in the 9th grade (Program of the chemistry course for 8-9 grades of educational institutions. Authors: NE Kuznetsova, IM Titova, NN Gara). Samples of the design of practical work with possible answers of students, instruction cards for practical work are given. Each practical work is accompanied by safety rules. Projected student responses are italicized.