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Frank Frank Class 10 Chemistry Part 2

Frank Class 10 Chemistry Part 2 - Shaalaa.com

Chapter 12: Practical Work

Exercise

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 307]

Exercise | Q 1.1 | Page 307

How will you identify?
Chloride ion

Exercise | Q 1.2 | Page 307

How will you identify?
Chlorine gas

Exercise | Q 1.3 | Page 307

How will you identify?
Sulphur dioxide gas

Exercise | Q 1.4 | Page 307

How will you identify?
A Soluble carbonate

Exercise | Q 1.5 | Page 307

How will you identify?
An amphoteric hydroxide

Exercise | Q 2.1 | Page 307

Name the following:
A green coloured carbonate.

Exercise | Q 2.2 | Page 307

Name the following:
A steel grey coloured solid non-metal.

Exercise | Q 2.3 | Page 307

Name the following:
A nitrate which has no water of crystallization.

Exercise | Q 2.4 | Page 307

Name the following:
A sulphate insoluble in water.

Exercise | Q 3.1 | Page 307

Give two tests of the following:
NH3

Exercise | Q 3.2 | Page 307

Give two tests of the following:
Oxygen

Exercise | Q 3.3 | Page 307

Give two tests of the following:
Water vapour

Exercise | Q 4 | Page 307

Write the steps needed for flame test ?

Exercise | Q 5.1 | Page 307

What happens when
NH3 solution is added to CuSO4 solution drop by drop and then in excess.

Exercise | Q 5.2 | Page 307

What happens when
Caustic soda solution is added to Cu(NO3)2 solution and product boiled.

Exercise | Q 5.3 | Page 307

What happens when
Common salt solution is added to silver nitrate solution and NH3 solution add to it.

Exercise | Q 5.4 | Page 307

What happens when
Lead nitrate solution treated with calcium chloride solution and products are heated and cooled.

Exercise | Q 6.1 | Page 307

Write sqauential observation for effect of heat on Copper nitrate.

Exercise | Q 6.2 | Page 307

Write sqauential observation for effect of heat on Lead carbonate.

Exercise | Q 6.3 | Page 307

Write sqauential observation for effect of heat on Ammonium chloride.

Exercise | Q 7 | Page 307

How will you distinguish between the two black samples, CuO and MnO2 with a chemical test?

Exercise | Q 8 | Page 307

A white solid A when heated with sodium hydroxide solution, gives a pungent gas B, which turns red litmus blue. The solid, when dissolved in dilute nitric acid and treated with silver nitrate gives a white precipitate of C which is soluble in an ammonia solution.

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 308]

Exercise | Q 1.1 | Page 308

Write the approximate colour of the following sample with the universal indicator:
Distilled water

Exercise | Q 1.2 | Page 308

Write the approximate colour of the following sample with the universal indicator: Acid rain

Exercise | Q 1.3 | Page 308

Write the approximate colour of the following sample with the universal indicator: Soap Solution

Exercise | Q 1.4 | Page 308

Write the approximate colour of the following sample with the universal indicator: Soil containing slaked lime

Exercise | Q 1.5 | Page 308

Write the approximate colour of the following sample with the universal indicator: Gastric juice

Exercise | Q 2.1 | Page 308

Using Sodium hydroxide solution, how would you distinguish: Ammonium sulphate from sodium sulphate.

Exercise | Q 2.2 | Page 308

Using Sodium hydroxide solution, how would you distinguish: Zinc nitrate solution from calcium nitrate solution.

Exercise | Q 2.3 | Page 308

Using Sodium hydroxide solution, how would you distinguish: Iron(II) chloride from Iron (III) chloride

Exercise | Q 3.1 | Page 308

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Sodium chloride solution and sodium nitrate solution.

Exercise | Q 3.1 | Page 308

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Sodium chloride solution and sodium nitrate solution.

Exercise | Q 3.2 | Page 308

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Sodium sulphate solution and sodium chloride solution.

Exercise | Q 3.3 | Page 308

One chemical test that would enable you to distinguish between the following pair of chemicals. Describe what happens with each chemical or state 'no visible reaction'.
Calcium nitrate solution and zinc nitrate solution.

Exercise | Q 4.1 | Page 308

State the effect of adding a small amount of : (a) sodium hydroxide (b) ammonium hydroxide followed by an excess in case to samples of the salt solutions.
Calcium nitrate [ small amount __________ in excess __________ ]

Exercise | Q 4.2 | Page 308

State the effect of adding a small amount of : (a) sodium hydroxide (b) ammonium hydroxide followed by an excess in case to samples of the salt solutions.
Zinc nitrate [ small amount ________ in excess ________]

Exercise | Q 4.3 | Page 308

State the effect of adding a small amount of : (a) sodium hydroxide (b) ammonium hydroxide followed by an excess in case to samples of the salt solutions.
Lead nitrate [ small amount ________ in excess ________ ]

Exercise | Q 5 | Page 308

State what do you observe when ammonium hydroxide to Iron (III) sulphate solution.

Exercise | Q 6 | Page 308

From the formulae listed below, Choose, one, corresponding to the salt having the given description:
AgCl, CuCO3, CuSO4.5H2O, KNO3, NaCl, NaHSO4, Pb(NO3)2, ZnCO3, ZnSO4, 7H2O.
On heating this, salt changes from green to black.

Exercise | Q 7.1 | Page 308

How would you distinguish between Zn2+ and Pb2+ using ammonium hydroxide solution?

Exercise | Q 7.2 | Page 308

Copy and complete the following table which refers to the action of heat on some carbonates :

Carbonate Colour of residue on cooling
Zinc carbonate  
Lead carbonate  
Copper carbonate  

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 309]

Exercise | Q 1.1 | Page 309

Write the observation for the following:
NaOH is added drop-wise till in excess to a solution of zinc sulphate.

Exercise | Q 1.2 | Page 309

Write the observation for the following :
NH4OH is added first in a small quantity and then in excess to a solution of copper sulphate.

Exercise | Q 1.3 | Page 309

Write the observation for the following:
Excess NH4OH is added to a substance obtained by adding hydrochloric acid in silver nitrate solution.

Exercise | Q 1.4 | Page 309

Write the observation for the following:
Moist starch iodide paper is put on the mouth of a test tube containing chlorine gas.

Exercise | Q 1.5 | Page 309

Write the observation for the following:
A paper dipped in potassium permanganate solution is put on the mouth of a test tube containing sulphur dioxide gas.

Exercise | Q 1.6 | Page 309

Write the observation for the following:
Decomposition of bicarbonates by dil. H2SO4
2NaHCO3 + H2SO4 → Na2SO4 + 2H2O + 2CO2
2KHCO3 + H2SO4 → K2SO4 + 2H2O + 2CO2

Exercise | Q 2 | Page 309

Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solutions of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy 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 precipitate when NaOH is added in a small quantity Nature of precipitate (soluble or insoluble) when NaOH is added in excess
Copper (II) sulphate (i) (vi)
Zinc nitrate (ii) (vii)
Lead nitrate (iii) (viii)
Calcium chloride (iv) (ix)
Iron (III) Sulphate (v) (x)
Exercise | Q 3 | Page 309

A solution of hydrogen chloride in water is prepared. The following substances are added to separate portions of the solution :

S.NO. Substance added Gas evolved Odour
1 Calcium carbonate _________ _________
2 Magnesium ribbon _________ _________
3 Manganese (IV) oxide with heating _________ _________
4 Sodium sulphide _________ _________
Exercise | Q 4 | Page 309

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 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 a 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 excess of ammonium hydroxide is added to it ?
(v) Which solution gives a white precipitate with excess ammonium hydroxide solution?

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 310]

Exercise | Q 1.1 | Page 310

State the colour of the residue formed when nitrates of :
1. Calcium
2. Zinc
3. Lead
4. Copper are strongly heat

Exercise | Q 1.2 | Page 310

Give one test to distinguish between the following pair of chemicals.
Sodium nitrate solution and sodium chloride solution.

Exercise | Q 1.2 | Page 310

Give one test to distinguish between the following pair of chemicals.
Iron (III) Chloride solution and copper chloride solution.

Exercise | Q 1.2 | Page 310

Give one test to distinguish between the following pair of chemical.
Zinc nitrate solution and calcium nitrate solution.

Exercise | Q 2 | Page 310

Match the following:

Column A  Column B
1. A substance that turns moist starch iodide paper blue. A. Ammonium sulphate
2. A compound which release a reddish brown gas on reaction with concentrated sulphuric acid and copper turnings.  B. Lead carbonate
3. A solution of this compound gives dirty green precipitate with sodium hydroxide. C. Chlorine
4. A compound which on heating with sodium hydroxide produces a gas which forms dense white fumes with hydrogen chloride. D. Copper nitrate
5. A white solid which gives a yellow residue on heating E. Ferrous sulphate
Exercise | Q 3 | Page 310

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. Tabulate your answers in the format given below:
(i) When silver nitrate solution is added to asolution of A, a white precipitate, insoluble in dilute nitric acid, is formed.
(ii) Addition of dilute hydrochloric acid to B produces a gas which turns lead acetate paper black.
(iii) 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, a brown ring is formed.
(iv) When dilute sulphuric acid is added to D, a gas is produced which turns acidified potassium dichromate solution from orange to green.
(v) Addition of dilute hydrochloric acid to E produces an effervescence. The gas produced turns limewater milky but does not affect acidified potassium dichromate solution.

Salt Anion
A  
B  
C  
D  
E  

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 311]

Exercise | Q 1 | Page 311

Choose the correct answer:
The salt which in solution gives a pale 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

Exercise | Q 2 | Page 311

Select from the list given (a to e) one substances in each case which matches the description given in parts (i) to (v). (Note : Each substance is used only one in the answer)
(a) Nitroso Iron (II) Sulphate
(b) Iron (III) chloride
(c) Chromium sulphate
(d) Lead (II) chloride
(e) Sodium chloride
(i) A compound which is deliquescent
(ii) A compound which is insoluble in cold water, but soluble in hot water
(iii) The compound responsible for the brown ring during the brown ring test of nitrate iron
(iv) A compound whose aqueous solution is neutral in nature
(v) The compound which is responsible for the green colouration when sulphur dioxide is passed through acidified potassium dichromate solution

Exercise | Q 3 | Page 311

What would you observe in the following cases:
Ammonium hydroxide is first added in a small quantity and then in excess to a solution of copper sulphate.

Exercise | Q 4 | Page 311

Sodium hydroxide solution is added to the solutions containing the ions mentioned in List X. List Y gives the details of the precipitate. Match the ions with their coloured precipitates.

List X List Y
(i) Pb2+ (A) Reddish Brown
(ii) Fe2+ (B) White insoluble inexcess
(iii) Zn2+ (C) Dirty green
(iv) Fe3+ (D) White soluble in excess
(v) Cu2+ (E) White soluble in excess
(vi) Ca2+ (F) Blue

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 312]

Exercise | Q 1.1 | Page 312

State two observations when
Lead nitrate crystals are heated in a hard glass test tube.

Exercise | Q 1.2 | Page 312

State two observations when
A few crystals of KNO3 are heated in a hard glass tube

Exercise | Q 2.1 | Page 312

Give a chemical test to distinguish between the following pair of compounds:
Sodium chloride solution and sodium nitrate solution

Exercise | Q 2.2 | Page 312

Give a chemical test to distinguish between the following pair of compounds:
Hydrogen chloride gas and hydrogen sulphide gas

Exercise | Q 2.3 | Page 312

Give a chemical test to distinguish between the following pair of compounds:
Calcium nitrate gas and sulphur diaoxide gas

Exercise | Q 2.4 | Page 312

Give a chemical test to distinguish between the following pair of compounds:
Carbon dioxide gas and sulphur dioxide gas

Exercise | Q 3 | Page 312

Distinguish between the following pairs of compounds using the test given with brackets :
Dilute sulphuric acid and dilute hydrochloric acid (using barium chloride solution)

Exercise | Q 4.1 | Page 312

State the inference drawn from the following observation :
On Carrying out the flame test with a salt P a brick red flame was obtained. What is the cation in P?

Exercise | Q 4.2 | Page 312

State the inference drawn from the following observation:
A gas Q turns moist lead acetate paper silvery black. Identify the gas Q.

Exercise | Q 4.3 | Page 312

State the inference drawn from the following observation:
pH of liquid R is 10. What kind of substance is R?

Exercise | Q 4.4 | Page 312

State the inference drawn from the following observations:
Salt S is prepared by reacting dilute sulphuric acid with copper oxide Identify S.

Exercise | Q 5.1 | Page 312

State your observation of the following case :
When dilute hydrochloric acid is added to sodium carbonate crystals.

Exercise | Q 5.2 | Page 312

State your observation of the following case :
When excess sodium hydroxide is added to calcium nitrate solution

Exercise | Q 5.3 | Page 312

State your observation of the following case :
At the cathode when acidified aqueous copper sulphate solution is electrolyzed with copper electrodes

Exercise | Q 5.4 | Page 312

State your observation of the following case :
When calcium hydroxide is heated with ammonium chloride crystals.

Exercise | Q 5.5 | Page 312

State your observation of the following case :
When moist starch iodide paper is introduced into chlorine gas.

Exercise | Q 6 | Page 312

The following table shows the tests a student performed on four different aqueous solutions which are X,Y,Z and W. Based on the observations provided, Identify the cation present

Chemical Test

Observation Conclusion
To Solution X, ammonium hydroxide is added in minium quantity first and then in excess A dirty white precipitate is formed which dissolves in excess to form a clear solution (i)
To Solution Y, ammonium hydroxide is added in minimum quantity first and then in excess A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution (ii)
To solution W, A small quantity of sodium hydroxide solution is added and then in excess A white precipitate is formed which remains insoluble (iii)
To a salt Z, calcium hydroxide solution is added and then heated A pungent smelling gas turning moist red litmus paper blue is obtained (iv)

Frank solutions for Class 10 Chemistry Chapter 12 Exercise [Page 313]

Exercise | Q 1.1 | Page 313

Identify the anion present of the following compound:
A salt M on treatment with concentrated sulphuric acid produces a gas which fumes in moist air and gives dense fumes with ammonia.

Exercise | Q 1.2 | Page 313

Identify the anion present of the following compound:
A salt D on treatment with dilute sulphuric acid produces a gas which turns lime water milky but has no effect on acidified potassium dichromate solution

Exercise | Q 1.3 | Page 313

Identify the anion present of the following compound:
When barium chloride solution is added to salt solution E a white precipitate insoluble in dilute hydrochloric acid is obtained

Exercise | Q 2 | Page 313

From the list of the following salts choose the salt that most appropriately fits the description given in the following :
[ AgCl, MgCl2, NaHSO4, PbCO3, ZnCO3, KNO3, Ca(NO3)2 ]

(i) A deliquescent salt
(ii) An insoluble chloride
(iii) On heating this salt gives a yellow residue when hot and white when cold
(iv) On heating this salt, a brown coloured to prepare the following salts:

Exercise | Q 3.1 | Page 313

Give balanced chemical equation to prepare the following salt:
Lead sulphate from lead carbonate

Exercise | Q 3.2 | Page 313

Give balanced chemical equation to prepare the following salt:
Sodium sulphate using dilute sulphuric acid

Exercise | Q 3.3 | Page 313

Give balanced chemical equation to prepare the following salt :
Copper chloride using copper carbonate

Exercise | Q 4.1 | Page 313

Identify the cation of the following case:
NaOH solution when added to solution (A) gives a reddish brown precipitate

Exercise | Q 4.2 | Page 313

Identify the cation of the following case:
NH4OH solution when added to solution (B) gives white ppt. which does not dissolve in excess.

Exercise | Q 4.3 | Page 313

Identify the cation of the following case:
NaOH solution when added to solution (C) gives white ppt. which insoluble in excess.

Exercise | Q 5.1 | Page 313

Identify the gas evolved and give the chemical test of the following case :
Dilute hydrochloric acid reacts with sodium sulphite

Exercise | Q 5.2 | Page 313

Identify the gas evolved and give the chemical test of the following case :
Dilute hydrochloric acid reacts with iron (II) sulphide

Exercise | Q 6.1 | Page 313

Identify the salts P and Q from the observation given below:
On performing the flame test salt P produces a lilac coloured flame and its solution gives a white precipitate with silver nitrate solution. Which is soluble in ammonium hydroxide solution.

Exercise | Q 6.2 | Page 313

Identify the salts P and Q from the observation given below:
When dilute HCl is added to a salt Q, a brisk effervescence is produced and the gas turns lime water milky. When NH4OH soltion is added to the above mixture (after adding dilute HCl), it produces a white precipitate which is soluble in excess NH4OH solution.

Chapter 12: Practical Work

Exercise

Frank Frank Class 10 Chemistry Part 2

Frank Class 10 Chemistry Part 2 - Shaalaa.com

Frank solutions for Class 10 Chemistry chapter 12 - Practical Work

Frank solutions for Class 10 Chemistry chapter 12 (Practical Work) include all questions with solution and detail explanation. This will clear students doubts about any question and improve application skills while preparing for board exams. The detailed, step-by-step solutions will help you understand the concepts better and clear your confusions, if any. Shaalaa.com has the CISCE Frank Class 10 Chemistry Part 2 solutions in a manner that help students grasp basic concepts better and faster.

Further, we at Shaalaa.com provide such solutions so that students can prepare for written exams. Frank textbook solutions can be a core help for self-study and acts as a perfect self-help guidance for students.

Concepts covered in Class 10 Chemistry chapter 12 Practical Work are Periodic Properties-chemical Reactivity, Relation Between Atomic Number for Light Elements (Proton Number) and Atomic Mass for Light Elements, Periodicity on the Basis of Atomic Number for Elements, Periodic Properties - Electronegativity, Periodic Properties - Electron Affinity, Periodic Properties - Ionisation Potential, Periodic Properties - Metallic Character, Periodic Properties - Atomic Size, Periodic Properties and Variations of Properties:- Physical and Chemical, Periodic Properties -physical Properties, Formation and Properties of Ionic Compounds, Concept of Coordinate Bond, Comparison of Electrovalent and Covalent Compounds, Characteristic Properties of Covalent Compounds, Concept of Covalent Bond, Characteristic Properties of Electrovalent Compounds, Structure of Electrovalent Compounds NaCl, MgCl2, CaO, Concept of Electrovalent, Concept of Chemical Bonding, Concept of Acids and Bases, Concept of Molecule, Preparation - Laboratory Preparation of Salts (Normal and Acid Salts) – Relevant Laboratory, General Properties of Salts:, Types of Salts, Use of Litmus and pH Paper to Test for Acidity and Alkalinity, Ions Present in Mineral Acids, Alkalis and Salts and Their Solutions, Action of Alkalis (Naoh, Koh) on Certain Metals, Their Oxides and Hydroxides, On Solution of Salts - Sodium Hydroxide on Ammonium Salts, On Solution of Salts - Special Action of Ammonium Hydroxide on Solutions of Copper Salt, Formation and Colour of Hydroxide Precipitated for Solutions of Salts of Ca, Fe, Cu, Zn and Pb, On Solution of Salts - Colour of Salt and Its Solution, Analytical Chemistry, Molar Volume of a Gas at S.T.P, Deduction of Simple (Empirical) and Molecular Formula from the Percentage Composition of a Compound, Vapour Density and Its Relation to Relative Molecular Mass:, Refer to the Atomicity of Hydrogen, Oxygen, Nitrogen and Chlorine, Avogadro’s Law of Volume, Gay Lussac’s Law of Combining Volumes, Mole Concept, Electrolytes and Non-Electrolytes, Substances Containing Molecules Only, Ions Only, Both Molecules and Ions., Electrolysis, An Elementary Study of the Migration of Ions, Applications of Electrolysis, Chemical Method - NaOH for Purifying Bauxite – Baeyer’s Process, Dressing of the Ore, Extraction of Aluminium, Common Ores of Iron, Aluminium and Zinc, Extracting Metals Towards the Top of the Activity Series, Extracting Metals in the Middle of the Activity Series, Extracting Metals Low in the Activity Series, Extraction of Metals, Reduction of Metallic Oxides, Concept of Metallurgy, Uses of Acetic Acid, Chemical Properties of Acetic Acid, Concept of Acetic Acid, Concept of Ethanol, Hydrocarbons - Alkynes, Hydrocarbons - Alkenes,, Hydrocarbons - Alkanes, Simple Nomenclature, Homologous Series, Structure of Compounds with Single, Double and Triple Bonds, Unique Nature of Carbon Atom, Concept of Organic Compounds, Catalytic Oxidation of Ammonia as the Source of Nitric Acid, Ammonia - Uses of Ammonia, Burning of Ammonia in Oxygen, Ammonia - Reactions with Hydrogen Chloride and with Hot Copper (Ii) Oxide and Chlorine, Aqueous Solution of Ammonia, Ammonia - Density and Solubility of Ammonia (Fountain Experiment), Ammonia - Manufacture by Haber’s Process;, Ammonia - Laboratory Preparation, Concept of Ammonia, Properties of Ammonia, Nitric Acid as an Oxidizing Agent., Nitric Acid - Laboratory Method of Preparation of Nitric Acid from Potassium Nitrate Or Sodium Nitrate, Concept of Nitric Acid, Hydrogen Chloride - Acidic Properties of Its Solution, Hydrogen Chloride - Reaction with Ammonia, Hydrogen Chloride - Density and Solubility of Hydrogen Chloride (Fountain Experiment), Hydrogen Chloride - Preparation of Hydrogen Chloride from Sodium Chloride, Concept of Hydrogen Chloride, Method of Preparation of Hydrochloric Acid, Precipitation Reactions with Silver Nitrate Solution and Lead Nitrate Solution, Non-volatile Nature of Sulphuric Acid, Sulphuric Acid-manufacture by Contact Process, Concept of Sulphuric Acid, Sulphuric Acid - Behaviour as an Acid When Dilute, Sulphuric Acid - Oxidizing Agent When Concentrated, Sulphuric Acid - Dehydrating Agent.

Using Frank Class 10 solutions Practical Work exercise by students are an easy way to prepare for the exams, as they involve solutions arranged chapter-wise also page wise. The questions involved in Frank Solutions are important questions that can be asked in the final exam. Maximum students of CISCE Class 10 prefer Frank Textbook Solutions to score more in exam.

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