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Chapters
2: Chemical Bonding
3: Acids, Bases and Salts
4: Analytical Chemistry: Uses of Ammonium Hydroxide and Sodium Hydroxide
5: Mole concept and Stoichiometry
6: Electrolysis
7: Metallurgy
8: Study of Compounds - Hydrogen Chloride
9: Study of Compounds - Ammonia
10: Study of Compounds - Nitric Acid
11: Sulphuric Acid
12: Organic Chemistry
▶ 13: Practical Work
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Solutions for Chapter 13: Practical Work
Below listed, you can find solutions for Chapter 13 of CISCE Selina for Concise Chemistry [English] Class 10 ICSE.
Selina solutions for Concise Chemistry [English] Class 10 ICSE 13 Practical Work Intext Questions [Page 224]
- Give only one suitable chemical test to identify the following gases.
- Ammonia
- Sulphur dioxide
- Hydrogen chloride
- Chlorine
- Carbon dioxide
- Oxygen
- Hydrogen
- Select a basic gas mentioned in Q. (a). How is the basic nature suspected?
- Select acidic gases from the gases mentioned in Q. (a). How is the acidic nature suspected?
- The two gases A and B are bleaching agents. A is greenish-yellow and bleaches due to its oxidizing property while B is a colourless gas that bleaches due to reduction. Identify A and B?
- Which gas turn blue cobalt chloride paper light pink?
Give one similarity in the test between- Cl2 and HCl
- SO2 and CO2.
Name the gases which extinguishes burning wooden splinter.
Name the gas which: Turns moist red litmus blue.
Name the gases which do not affect moist litmus.
Name the gas which: Affects the acidified K2Cr2O7 paper and also turns lime water dirty milky.
Name two carbonates do not produce carbon dioxide on heating.
Name A colourless gas which bleaches.
Name gases which has a sour taste.
Name greenish-yellow gas which also bleaches.
Name gas with rotten egg smell.
Selina solutions for Concise Chemistry [English] Class 10 ICSE 13 Practical Work Exercise 13 [Pages 228 - 230]
From the following list of substances choose those which meet the description given below.
Ammonium chloride, ammonium nitrate, chlorine, dilute hydrochloric acid, iron, lead nitrate, manganese (IV) oxide, silver nitrate, sodium nitrate, sodium nitrite, and sulphur.
Two compounds whose aqueous solutions give white precipitates with dilute hydrochloric acid.
Name the anion present in the following compound:
Compound A, when warmed with concentrated sulphuric acid, gives a gas which fumes in moist air and which gives dense white fumes with ammonia.
Name the anion present in the following compound:
When a barium chloride solution is added to a solution of compound B, a white precipitate insoluble in dilute hydrochloric acid is formed.
Name the anion present in the following compound:
The action of heat on the insoluble compound C produces a gas which turns lime water turbid.
Name the anion present in the following compound:
Compound D, when warmed with dilute sulphuric acid, gives a gas that turns acidified dichromate solution green.
A given white crystalline salt was tested as follows:
It dissolved in water and the resulting solution of the salt turned blue litmus red. What conclusions can be drawn for the observation?
A given white crystalline salt was tested as follows:
The addition of barium chloride solution into this solution gave a white precipitate. What conclusions can be drawn for the observation?
A given white crystalline salt was tested as follows:
A flame test on the salt gave a persistent golden-yellow colourisation. What conclusions can be drawn for the observation?
Sodium hydroxide solution is added to solution A. A white precipitate is formed which is insoluble in excess sodium hydroxide solution. What is the metal ion present in solution A?
When an ammonium hydroxide solution is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide giving an inky blue solution. What is the cation present in solution B?
When an ammonium salt is warmed with sodium hydroxide solution, a gas is evolved. State three ways in which you could identify this gas.
Complete the following table and write your observations.
| Hydrogen sulphide | Ammonia | Sulphur dioxide | Hydrogen chloride | |
| Shake the gas with red litmus solution |
Complete the following table and write your observations.
| Hydrogen sulphide | Ammonia | Sulphur dioxide | Hydrogen chloride | |
| Shake the gas with blue litmus solution |
Complete the following table and write your observations.
| Hydrogen sulphide | Ammonia | Sulphur dioxide | Hydrogen chloride | |
| Apply a burning splint to the gas |
Use the information given in (a) to (h) to identify the substances P to W selecting your answers from the given list.
List:
| Calcium | Oxygen | Copper (II) Oxide |
| Carbon | Calcium hydroxide | Copper (II) Nitrate |
| Lead (II) Oxide | Hydrogen chloride | Chlorine |
| Lead (II) Nitrate | Calcium Oxide | Ammonium chloride |
- P is white solid. When heated produces white fumes (sublime).
- P and R on warming produce an alkaline gas.
- On adding water to T, heat is evolved and R is formed.
- Q burns brightly in the air to form T.
- When S is heated, it gives off brown fumes and leaves a black residue of U.
- A solution of S is formed by warming U with dilute nitric acid.
- V is a gaseous non-metallic element that reacts with hydrogen to form W.
- A solution of W will neutralize the solution of R.
Copy and complete the following table which refers to the action of heat on the carbonate:
| Carbonate | Colour of residue on cooling |
| Zinc Carbonate |
Copy and complete the following table which refers to the action of heat on the carbonate:
| Carbonate | Colour of residue on cooling |
| Lead carbonate |
Copy and complete the following table which refers to the action of heat on the carbonate:
| Carbonate | Colour of residue on cooling |
| Copper carbonate |
Distinguish by a chemical test, Sodium carbonate and sodium sulphite.
Distinguish by a chemical test sodium chloride and sodium sulphite.
Distinguish by a chemical test sodium hydroxide solution and ammonium hydroxide solution.
Distinguish by a chemical test, ammonium sulphate and sodium sulphate.
Distinguish by a chemical test, sulphuric acid from nitric acid and hydrochloric acid.
Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solution of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy of the following table and write the colour of the precipitate in (i) to (v) and the nature of the precipitate (soluble or insoluble) in (vi) to (x).
|
Aqueous salt solution |
Colour of the precipitate when NaOH is added in small quantity |
Nature of the(soluble or insoluble) when NaOH is added in excess |
|
copper (II) sulphate zinc nitrate lead nitrate calcium chloride Iron (III) sulphate |
(i) (ii) (iii) (iv) (v) |
(vi) (vii) (viii) (ix) (x) |
State your observation when lead nitrate solution and sodium chloride solution are mixed.
State your observation when zinc chloride solution, zinc nitrate solution, and zinc sulphate solutions are added individually to barium chloride solution.
State your observations when zinc chloride solution, zinc nitrate solution, and zinc sulphate solutions are added individually to lead nitrate solution.
State your observation when:
Decomposition of bicarbonates by dil. H2SO4
2NaHCO3 + H2SO4 → Na2SO4 + 2H2O + 2CO2
2KHCO3 + H2SO4 → K2SO4 + 2H2O + 2CO2
Write the observation for the following:
Decomposition of bicarbonates by dil. H2SO4
\[\ce{2KHCO3 + H2SO4 -> K2SO4 + 2H2O + 2CO2}\]
The questions (i) to (v) refer to the following salt solutions listed A to F.
A.Copper Nitrate
B.Iron (II) Sulphate
C.Iron (III) chloride
D.Lead Nitrate
E.Magnesium sulphate
F.Zinc chloride
(I)Which two solutions will give a white precipitate when treated with dilute hydrochloric acid followed by a barium chloride solution?
(II)Which two solutions will give a white precipitate when treated with dilute nitric acid followed by silver nitrate solution?
(III)Which solution will give white precipitate, when either dilute hydrochloric acid or dilute sulphuric acid is added to it?
(IV)Which solution becomes a deep/inky blue colour when the excess of ammonium hydroxide is added to it?
(V)Which solution gives a white precipitate with an excess of ammonium hydroxide solution?
Mention the colour change observed when the following indicator is added:
| Solution | Acids | Alkalies |
| Alkaline phenolphthalein solution |
Mention the colour change observed when the following indicator is added:
| Solution | Acids | Alkalies |
| Methyl orange solution |
Mention the colour change observed when the following indicator is added:
| Solution | Acids | Alkalies |
| Neutral litmus solution |
Salts A, B, C, D, and E undergo reactions (i) to (v) respectively. Identify the anion present in these salts on the basis of these reactions.
- When silver nitrate solution is added to a solution of A, a white precipitate, insoluble in dilute nitric acid, is formed.
- The addition of dilute hydrochloric acid to B produces a gas which turns lead acetate black paper.
- When a freshly prepared solution of ferrous sulphate is added to a solution of C and concentrated sulphuric acid is gently poured from the side of the test-tube, a brown ring is formed.
- When dilute sulphuric acid is added to D, a gas is produced which turns acidified potassium dichromate solution from orange to green.
- The addition of dilute hydrochloric acid to E produces effervescence. The gas produced turns lime water milky but does not affect acidified potassium dichromate solution.
The salt which in solution gives a pale green precipitate with sodium hydroxide solution and a white precipitate with barium chloride solution is ______.
Iron (III) sulphate
Iron (II) sulphate
Iron (II) chloride
Iron (III) chloride
Identify the following substance:
An alkaline gas A which gives dense white fumes with hydrogen chloride.
Identify the following substance:
A dilute acid B, which does not normally give hydrogen when reacted with metals but does give a gas when it reacts with copper.
Identify the following substance:
Gas C has an offensive smell like rotten eggs.
Identify the following substance:
Gas D is a colourless gas which can be used as a bleaching agent.
Identify the following substance:
Liquid E can be dehydrated to produce ethene.
Solutions for 13: Practical Work
Selina solutions for Concise Chemistry [English] Class 10 ICSE chapter 13 - Practical Work
Shaalaa.com has the CISCE Mathematics Concise Chemistry [English] Class 10 ICSE CISCE solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. Selina solutions for Mathematics Concise Chemistry [English] Class 10 ICSE CISCE 13 (Practical Work) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
Further, we at Shaalaa.com provide such solutions so students can prepare for written exams. Selina textbook solutions can be a core help for self-study and provide excellent self-help guidance for students.
Concepts covered in Concise Chemistry [English] Class 10 ICSE chapter 13 Practical Work are Group I (Alkali Metals), Group VIIA Or Group 17 (The Halogens), History of Periodic Table: Early Attempts at the Classification of Elements, Dobereiner’s Triads, Newland's Law of Octaves, Mendeleev’s Periodic Table, The Modern Periodic Table, Periodic Properties, Shells (Orbits), Valency, Atomic Radius Or Atomic Size, Metallic and Non-metallic Characters, Ionisation Potential (Ionisation Energy), Electron Affinity, Electronegativity, Atomic Number (Z), Mass Number (A), and Number of Neutrons (n), Atomic Mass, Study of Specific Groups in Periodic Table, Chemical Reactivity, Types of Covalent Bond, Formation of Covalent Bond, Formation of Coordinate Bond, Chemical Bond, The Covalent Bond, Properties and Comparison of Electrovalent and Covalent Compounds, Coordinate Bond, Ionic or Electrovalent Bond, Ionic or Electrovalent Bond, Types of Chemical Bond, Effect of Electricity on Electrovalent and Covalent Compounds, Acids, Making of natural indicator, Salts, Classification of Salts, Methods of Preparation of Soluble Salts, Preparation of Insoluble Salts, Classification of Acids, Preparation of Acids, Properties of Acids, Uses of Acids, Bases (Alkalis), Classification of Bases (Alkalis), Preparation of Bases, Properties of Bases (Alkalis), Uses of Bases, Strength of Acidic or Basic Solutions, Laboratory Preparation of Some Salts, Laboratory Preparation of Iron (III) Chloride, Laboratory Preparation of Zinc Sulphate Crystals from Zinc and Sulphuric Acid, Laboratory Preparation of Lead Chloride and Calcium Carbonate, Laboratory Preparation of an Acid Salt Sodium Bicarbonate, Neutralisation, Laboratory Preparation of Copper (II) Sulphate (Or Blue Vitriol), Laboratory Preparation of Sodium Sulphate Crystals, Properties of Salts, Analytical Chemistry, Action of Sodium Hydroxide Solution on Certain Metallic Salt Solutions, Action of Ammonium Hydroxide on Certain Salt Solutions, Action of Alkalis on Certain Metals, Action of Alkalis on Metal Oxides, Colours of the Salts and Their Solutions, Preferential Or Selective Discharge of Ions at Electrodes, Examples of Electrolysis, Electrolysis of Molten Lead Bromid, Electrolysis of Acidified Water Using Platinum Electrodes, Electrolysis of Copper Sulphate Solution Using Platinum Anode and Copper Or Platinum Cathode, Electrolysis of Aqueous Copper Sulphate - Using Copper Electrodes, Applications of Electrolysis, Electrolysis, Electrolytes, Nonelectrolyte, Electrochemical Cells, Electrodes, Oxidation, Reduction and Redox Reactions, Arrhenius Theory of Electrolytic Dissociation, Electrochemical Series, Mineral Resources, Types of Element: Non-metal, Ores, Extraction of Reactive Metals, Types of Element: Metals, Corrosion of Metals, Metallurgy, Types of Separation or Concentration of an Ore, Conversion of Concentrated Ore to Its Oxide, Reactivity Series of Metals, Reduction of Metal Oxides to Metals, Refining of Metals, Metallurgy of Aluminium, Extraction of Aluminium, Refining of Aluminium, Alloy, Making Alloys, Some Common Alloys, Prevention of Corrosion, Special Features of Carbon, Functional Groups in Carbon Compounds, Laboratory Preparation of Methane, Ethene (Ethylene), Laboratory Preparation of Ethyne, Organic Compounds, Organic Compounds in Daily Life, Hydrocarbons, Ethane, Preparation of Ethene (Ethylene), Alcohol, Ethanol, Laboratory Preparation of Ethanol, Classification of Organic Compound Based on the Kind of Atoms, Homologous Series of Carbon Compound, Classification of Organic Compounds Based on the Pattern of Carbon Chain, IUPAC Nomenclature of Hydrocarbons, Hydrocarbons: Alkynes, Ethyne, Nomenclature of Organic Compounds, Carbon: A Versatile Element, Classification of Compounds of Carbon, IUPAC Nomenclature of other classes, Alkyl Group, Isomers, Hydrocarbons: Alkanes, Methane, Laboratory Preparation of Ethane, Hydrocarbons: Alkenes, Carboxylic Acids, Ethanoic Acid, Ammonia, Physical Properties of Ammonia, Chemical Properties of Ammonia, Uses of Ammonia, Laboratory Preparation of Ammonia Gas, Preparation of Aqueous Ammonia, Manufacture of Ammonia (Haber's Process), General Methods of Preparation of Ammonia Gas, Tests for Ammonia Gas and Ammonium Ion, Laboratory Preparation of Nitric Acid, Manufacture of Nitric Acid, Nitric Acid, Physical Properties of Nitric Acid, Chemical Properties of Nitric Acid, Uses of Nitric Acid, Tests for Nitric Acid and Nitrates, Effects of Heat on Nitrates, Hydrogen Chloride, Hydrochloric Acid, Uses of Hydrochloric Acid, General Preparation of Hydrogen Chloride Gas, Laboratory Preparation of Hydrogen Chloride Gas, Physical Properties of Hydrogen Chloride Gas, Chemical Properties of Hydrogen Chloride Gas, Laboratory Method of Preparation of Hydrochloric Acid, Properties of Hydrochloric Acid, Tests for Hydrogen Chloride and Hydrochloric Acid, Sulphuric Acid, Manufacture of Sulphuric Acid (Constant Process), Chemical Properties of Sulphuric Acid, Preparation of Sulphuric Acid, Physical Properties of Sulphuric Acid, Uses of Sulphuric Acid, Tests for Sulphuric Acid and Sulphates, Percentage Composition, Empirical and Molecular Formula, Empirical Formula of a Compound, Determination of Empirical Formula, Determination of Molecular Formula, Chemical Equation, Balancing Chemical Equation, Numerical Problems of Chemical Equation, The Gas Laws, Fundamental Laws of Gases, Pressure and Volume Relationship or Bolye's Law, Temperature - Volume Relationship or Charles's Law, Gas Equation, Standard Temperature Pressure (S.T.P.), Absolute Zero, Gay Lussac’s Law of Combining Volumes, Avogadro’s Law, Atomic Mass, Molecular Mass, Mole Concept, Relationship Between Vapour Density and Relative Molecular Mass, Laboratory Preparation of Hydrogen, Laboratory Preparation of Oxygen, Laboratory Preparation of Carbon Dioxide, Laboratory Preparation of Chlorine, Laboratory Preparation of Hydrogen Chloride Gas, Laboratory Preparation of Sulphur Dioxide, Laboratory Preparation of Hydrogen Sulphide, Laboratory Preparation of Ammonia Gas, Laboratory Preparation of Water Vapour, Laboratory Preparation of Nitrogen Dioxide, Action of Heat on a Given Substance, Action of Dilute Sulphuric Acid on a Given Substance, Dry Test, Recognition of Substances by Colour, Recognition of Substances by Odour, Recognition of Substances by Physical State, Recognition of Substances by Action of Heat, Flame Test, Strength of Acidic or Basic Solutions, Indicators, Identification of Ions, Identification of Cations, Identification of Anions, Distinction Between Colourless Solutions of Dilute Acids and Alkalis, Distinguish Between Black Copper Oxide and Black Manganese Dioxide, Laboratory Preparation of Hydrogen, Laboratory Preparation of Oxygen, Laboratory Preparation of Carbon Dioxide, Laboratory Preparation of Chlorine, Laboratory Preparation of Hydrogen Chloride Gas, Laboratory Preparation of Sulphur Dioxide, Laboratory Preparation of Hydrogen Sulphide, Laboratory Preparation of Ammonia Gas, Laboratory Preparation of Water Vapour, Laboratory Preparation of Nitrogen Dioxide, Action of Heat on a Given Substance, Action of Dilute Sulphuric Acid on a Given Substance, Dry Test, Recognition of Substances by Colour, Recognition of Substances by Odour, Recognition of Substances by Physical State, Recognition of Substances by Action of Heat, Flame Test, Strength of Acidic or Basic Solutions, Indicators, Identification of Ions, Identification of Cations, Identification of Anions, Distinction Between Colourless Solutions of Dilute Acids and Alkalis, Distinguish Between Black Copper Oxide and Black Manganese Dioxide.
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