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ICSE Class 10 Chemistry Chapter 13 Practical Work Digital Edition
For Class 10 Chemistry, this chapter in ICSE Class 10 Chemistry Chapter 13 Practical Work provides a detailed overview of important concepts. We highly recommend using this text alongside the ICSE Solutions for Class 10 Chemistry to learn the exercise questions provided at the end of the chapter.
Chapter 13 Practical Work ICSE Book Class Class 10 PDF (2026-27)
13. Practical Work
Syllabus
Internal Assessment Of Practical Work
Candidates will be asked to observe the effect of reagents and/or of heat on substances supplied to them. The exercises will be simple and may include the recognition and identification of certain gases and ions listed below. The examiners will not, however, be restricted in their choice to substances containing the listed ions.
Gases: Hydrogen, Oxygen, Carbon dioxide, Chlorine, Hydrogen chloride, Sulphur dioxide, Hydrogen sulphide, Ammonia, Water vapour, Nitrogen dioxide.
Ions: Calcium, Copper, Iron, Lead, Zinc and Ammonium, Carbonate, Chloride, Nitrate, Sulphide, Sulphite and Sulphate.
Knowledge of a formal scheme of analysis is not required. Semi-micro techniques are acceptable but candidates using such techniques may need to adapt the instructions given to suit the size of the apparatus being used.
Candidates are expected to have completed the following minimum practical work.
1. Make a solution of the unknown substance - add sodium hydroxide solution or ammonium hydroxide solution, make observations and give your deduction. Warming the mixture may be needed. Choose from substances containing Ca2+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+, NH4+.
2. Supply a solution of a dilute acid and alkali. Determine which is acidic and which is basic, giving two tests for each.
3. Add concentrated hydrochloric acid to each of the given substances, warm, make observations, identify any product and make deductions:
(a) copper oxide (b) manganese dioxide.
4. Use of pH in soil analysis, water analysis, medical field - simple identification with universal indicator.
13.1 Recognition And Identification Of Gases
| Preparation Of Gases | Recognition And Identification Of Gas |
|---|---|
1. Hydrogen Add dilute HCl or dilute H2SO4 to the reactive metals (metals above hydrogen in the activity series) like magnesium, zinc, iron, etc. Active metal + dil Acid - Salt + Hydrogen Mg + H2SO4 - MgSO4 + H2 Zn + 2HCl - ZnCl2 + H2 | (a) The evolved gas is colourless, odourless and neutral to litmus. (b) Pure hydrogen burns with a pale blue flame when a burning splint is brought near it. (c) Hydrogen-air burns with a pop sound when a burning taper is brought near it. |
2. Oxygen Heat higher metallic oxides or metal nitrates Heavy metal oxide - Metal oxide/ + oxygen 2Pb3O4 - 6PbO + O2 2HgO - 2Hg + O2 Metal nitrates - Metal oxide + Nitrogen + Oxygen dioxide 2Cu(NO3)2 - 2CuO + 4NO2 + O2 2Zn(NO3)2 - 2ZnO + 4NO2 + O2 | (a) The gas is colourless, odourless and neutral to litmus. (b) It rekindles a glowing splinter. (c) The gas is absorbed in colourless alkaline solution of pyrogallol and turns it dark brown. |
Teacher's Note
Oxygen is essential for combustion and respiration in daily life - this is why burning objects rekindle when oxygen is present, and why we breathe air which contains it.
| Preparation Of Gases | Recognition And Identification Of Gas |
|---|---|
3. Carbon dioxide Heat metallic carbonate (except sodium carbonate and potassium carbonate) or add dilute acid to any carbonate or hydrogen carbonate. Metallic carbonate - Metal oxide + carbon dioxide ZnCO3 - ZnO + CO2 CuCO3 - CuO + CO2 Metal carbonate/ + Acid - Salt + Water + Carbon dioxide hydrogen carbonate (dil) CaCO3 + 2HCl - CaCl2 + H2O + CO2 NaHCO3 + HCl - NaCl + H2O + CO2 | (a) The gas is colourless and odourless. (b) It turns moist blue litmus faint red. (c) When the gas is passed through the lime water, it turns milky due to the formation of white precipitate of calcium carbonate. Ca(OH)2 + CO2 - CaCO3 + H2O The milkiness disappears on passing excess of CO2 CaCO3 + CO2 + H2O - Ca(HCO3)2 (soluble) ppt (d) The gas has no effect on filter paper dipped in acidified K2Cr2O7 or KMnO4. |
4. Chlorine Add conc. HCl to oxidising agents like Pb3O4, PbO2, MnO2, etc. Oxidising + Conc. - Metal + Water + Chlorine agent HCl chloride Pb3O4 + 8HCl - 3PbCl2 + 4H2O + Cl2 MnO2 + 4HCl - MnCl2 + 2H2O + Cl2 | (a) The gas is greenish yellow having a sharp pungent choking odour. (b) It turns a moist blue litmus paper red and finally bleaches i.e., decolourises it. Cl2 + H2O - HCl + HClO HClO - HCl + [O] Colouring + matter bleached product (c) It turns moist starch iodide paper (KI + Starch solution) blue black. Cl2 + 2KI - 2KCl + I2 Starch + I2 - Blue black colour (d) Pass the gas through silver nitrate solution, a white ppt. is formed. |
5. Hydrogen chloride Add conc. H2SO4 to metal chlorides like NaCl, KCl, etc. Metal + Conc. sulphuric - Metal + Hydrogen chloride chloride acid sulphate NaCl + H2SO4 - NaHSO4 + HCl KCl + H2SO4 - KHSO4 + HCl | (a) The gas is colourless with a pungent choking odour. (b) The gas turns moist blue litmus paper red. (c) If a glass rod dipped in ammonia solution is brought near the gas, white fumes of ammonium chloride are formed. NH3(aq) + HCl - NH4Cl (d) Gas when passed through silver nitrate solution a white precipitate is formed. AgNO3(aq) + HCl - AgCl + HNO3 The ppt dissolves in excess of NH3OH. AgCl + 2NH3OH - Ag(NH3)2Cl + 2H2O soluble compound |
6. Sulphur dioxide Add dil. HCl or dil. H2SO4 to metallic sulphites. Metal sulphite/ + dil Acid - Salt + Water + Sulphur dioxide hydrogen sulphite Na2SO3 + 2HCl - 2NaCl + H2O + SO2 Na2SO3 + H2SO4 - Na2SO4 + H2O + SO2 2NaHSO3 + H2SO4 - Na2SO4 + 2H2O + 2SO2 | (a) The gas is colourless with a smell of burning sulphur i.e., suffocating odour. (b) It turns moist blue litmus red and finally bleaches it. (c) The gas turns lime water turbid (milky). (Similar to carbon dioxide). Ca(OH)2 + SO2 - CaSO3 + H2O (d) It decolourises pink potassium permanganate solution. 2KMnO4 + 2H2O + 5SO2 - K2SO4 + 2MnSO4 + 2H2SO4 (pink) (colourless) (e) It changes orange/yellow solution of acidified potassium dichromate green. K2Cr2O7 + H2SO4 + 3SO2 - Cr2(SO4)3 + K2SO4 + H2O (orange) (green) (f) It has no effect on lead acetate paper. |
Teacher's Note
Sulphur dioxide is released when we burn coal and oil for energy - this pollutes the air and is why acid rain occurs in industrial areas.
| Preparation Of Gases | Recognition And Identification Of Gas |
|---|---|
7. Hydrogen sulphide Add dil HCl or dil H2SO4 to metallic sulphides like ZnS, FeS. Metal + dil Acid - Salt + Hydrogen sulphide sulphide FeS + H2SO4 - FeSO4 + H2S ZnS + 2HCl - ZnCl2 + H2S | (a) The gas is colourless having a foul smell of rotten eggs. (b) It turns moist blue litmus red. (c) It turns lead acetate paper black. (CH3COO)2Pb + H2S - PbS + 2CH3COOH (black) (d) It also turns lead nitrate solution black. Pb(NO3)2 + H2S - PbS + 2HNO3 |
8. Ammonia Add alkali to ammonium salt like ammonium chloride, ammonium sulphate. Ammonium salt + Alkali - Salt + Water + Ammonia 2NH4Cl + Ca(OH)2 - CaCl2 + 2H2O + 2NH3 NH4Cl + NaOH - NaCl + H2O + NH3 | (a) The gas is colourless with a sharp pungent characteristic smell. (b) It turns moist red litmus blue. (c) If a glass rod dipped in conc. HCl is brought near the gas, dense white fumes of ammonium chloride are formed. (d) The gas turns colourless Nesslers reagent i.e. (K2HgI4) potassium mercuric iodide brown. |
9. Water vapour Heat a crystalline substance like hydrated sodium carbonate or hydrated copper sulphate. Hydrated salt - Anhydrous salt + Water vapour Na2CO3-10H2O - Na2CO3 + 10H2O CuSO4-5H2O - CuSO4 + 5H2O (blue) (white) | (a) Colourless, odourless forms a clear liquid on the cooler parts of the test-tube. (b) The liquid is neutral to litmus. (c) This liquid turns anhydrous copper sulphate from white to blue. CuSO4 + 5H2O - CuSO4-5H2O (white) (blue) (d) It turns blue cobalt chloride paper pink. CoCl2 + 6H2O - CoCl2-6H2O (blue) (pink) |
10. Nitrogen dioxide Heat heavy metal nitrate like copper nitrate, lead nitrate. Metal nitrate - Metal oxide + Oxygen + Nitrogen dioxide 2Cu(NO3)2 - 2CuO + O2 + 4NO2 2Pb(NO3)2 - 2PbO + O2 + 4NO2 Note - Sodium nitrate and potassium nitrate do not produce nitrogen dioxide on heating | (a) The gas is brown in colour having an irritating (pungent) odour and non-combustible. (b) It turns moist blue litmus paper red. (c) It turns starch iodide paper from colourless to blue black. 2KI + 2NO2 - 2KNO3 + I2 Turns potassium iodide paper brown. (d) It turns green acidified ferrous sulphate solution brown. |
Teacher's Note
Nitrogen dioxide is produced in car exhaust fumes and contributes to smog in cities - this is why we see brown haze over polluted urban areas on sunny days.
13.2 Recognition Of Substances By Colour, Odour, Physical State And Action Of Heat
A. Colour:
1. Blue or bluish green colour. Suspected ion: Cu2+
2. Light green colour. Suspected ion: Fe2+
3. Yellow or yellowish brown. Suspected ion: Fe3+
4. White colour (or colourless). Suspected ion: Pb2+, Zn2+, Ca2+, Na+, K+, or NH4+
B. Odour:
1. Smell of ammonia gas. NH4+
2. Smell of hydrogen sulphide gas. S2-
3. Smell of sulphur dioxide gas. SO3 2-
C. State:
1. Amorphous salt. CO3 2-
2. Hygroscopic or deliquescent nature. Cl- or NO3-
D. Action Of Heat:
1. Ammonium salt when heated with alkali (except ammonium hydroxide) produces Ammonia gas. Ammonium nitrate (explosive) and Ammonium chloride leaves no residue behind on heating. Ammonium dichromate on heating leaves greenish grey mass.
(NH4)2 Cr2O7 - Cr2O3 + N2 + 4H2O
(orange) (greenish grey)
2. PbO2, Pb3O4, HgO, KNO3, NaNO3 on heating produces oxygen gas.
3. Carbonate and bicarbonate on heating evolves carbon dioxide (except K2CO3 and Na2CO3).
4. Hydrated salts on heating produces water vapour.
5. Sulphites and some sulphates when heated produce sulphur dioxide gas.
6. Lead compounds decompose to give lead monoxide PbO (litharge). PbO is brown when hot, yellow when cold and sticks to the glass test tube.
7. Zinc compounds decompose on heating to give zinc oxide. ZnCO3 - ZnO + CO2
Zinc oxide is yellow when hot, white when cold. ZnO - ZnO
8. Copper compounds decompose to give black copper oxide. CuCO3 - CuO + CO2
(green) (black)
Note: Dry test involves - colour, density, physical state, dry heating and flame test. Wet test involves adding reagents to identify the substance.
Teacher's Note
When we heat hydrated copper sulphate crystals in a test tube, we can observe color change from blue to white - this reversible reaction shows the importance of water in determining mineral colors.
| Cation / Anion | K | Na | Ba | Ca | Mg | Al | Zn | Fe | Fe | Mn | Pb | Cu | Ag | Hg |
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| (I) | (I) | (II) | (II) | (II) | (III) | (II) | (II) | (III) | (II) | (II) | (II) | (I) | (II) | |
| NO3(I) | S | S | S | S | S | S | S | S | S | S | S | S | S | S |
| CH3COO(I) | S | S | S | S | S | Sp | S | S | S | S | S | S | S | S |
| Cl(I) | S | S | S | S | S | S | S | S | S | S | N | S | N | N |
| SO4(II) | S | S | N | Sp | S | S | S | S | S | S | N | S | Sp | S |
| OH(I) | S | S | S | Sp | Sp | N | N | N | N | N | N | N | - | - |
| S(II) | S | S | S | Sp | S | - | N | N | - | N | N | N | N | N |
| SO3(II) | S | S | N | N | N | - | N | - | N | N | N | N | N | N |
| PO4(III) | S | S | N | N | N | N | N | N | N | N | N | N | N | N |
| CO3(II) | S | S | N | N | N | - | N | N | N | N | N | N | N | N |
Note: S - Soluble; N - Insoluble; - Does not exist; Sp - Sparingly soluble
13.3 Identification Of Ions
Identification of ions is usually done in solution state.
Salt is dissolved in water to make solution. If the salts do not dissolve in water then Nitric acid is added to form nitrate. All nitrates are soluble in water.
Cations are tested by the action of alkalis as they give characteristic coloured metallic hydroxide precipitates (see chapter 4). When adding the alkali, add it slowly at first (one drop at a time). If it is added too quickly, it is easy to miss a precipitate that redissolves in excess.
Anions are tested by the reaction of acids or by specific reagents.
Identification Of Cations By Action Of Alkalis (See Chapter 4 Also)
| Sodium hydroxide solution | Ammonia solution | ||
|---|---|---|---|
| Metal | Colour of precipitate / With excess sodium hydroxide solution | Metal | Colour of precipitate / With excess ammonium hydroxide solution |
| Calcium | White curdy / Insoluble | Calcium | No ppt. / No change |
| Lead | White chalky / Soluble | Lead | White chalky / Insoluble |
| Zinc | White gelatinous / Soluble | Zinc | White gelatinous / Soluble |
| Copper | Pale blue / Insoluble | Copper | Pale blue / Soluble - deep blue solution |
| Iron (II) | Pale green turning brown / Insoluble | Iron (II) | Pale green turning brown / Insoluble |
| Iron (III) | Reddish brown / Insoluble | Iron (III) | Rust (brown) / Insoluble |
Test For Nh4+ Salt
(i) When caustic alkali (NaOH or KOH) is added to any ammonium salt, ammonia gas is evolved.
(ii) If Nessler's reagent is added to any ammonium salt solution, it turns brown.
Identification Of Anions
By Adding Dilute Sulphuric Acid
| Experiment | Observation | Inference |
|---|---|---|
1. (a) Take a small quantity of salt in a test tube and add dilute H2SO4. Warm, if no action in cold. (b) Pass the gas through lime water. (c) To the above precipitate, pass the gas in excess or add dilute nitric acid in excess. | Brisk effervescence and a colourless and odourless gas evolved. It does not support combustion i.e., burning splinter get extinguished. It turns moist blue litmus faint red. Lime water turns milky. The white precipitate dissolves to form colourless solution. | The gas evolved is carbon dioxide. The salt contains Carbonate ion (CO3 2-). |
2. (a) Take a small quantity of salt in a test-tube and add dil. H2SO4 acid. (b) Bring a moist lead acetate paper near the gas. | Rotten egg smelling gas evolved. It turns moist blue litmus paper red. Moist lead acetate paper turns black. | The gas evolved is hydrogen Sulphide. The salt contains Sulphide ion (S2-). |
3. (a) Take a small quantity of salt in a test-tube and add dilute H2SO4 acid (warm if necessary). (b) Bring a filter paper moistened with acidified K2Cr2O7 (Potassium dichromate) near the gas. | Gas evolved has suffocating odour of burning sulphur. Golden yellow or orange colour paper turns green. | The gas evolved is Sulphur dioxide. The salt contains Sulphite ion (SO3 2-). |
Teacher's Note
In the kitchen, baking soda reacts with dilute acids (like vinegar) to produce carbon dioxide gas bubbles - this is the same gas identification principle we use in the chemistry lab.
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