Class 10 FRANK Solutions Chemistry Chapter 3 - Study Of Acids, Bases and Salts

Revise Frank Solutions for ICSE Class 10 Chemistry Chapter 3 Study of Acids, Bases and Salts at TopperLearning. In this Chemistry chapter, study about volatile acids, weak dibasic acids, strong monobasic acids, alkali, base and other topics. Also, learn the various methods to prepare salts such as zinc sulphate, sodium sulphate etc.

In this chapter, learn the right chemical equations to explain reactions like conversion of hydrogen chloride to anhydrous iron (III) chloride. For more Chemistry practice, explore our ICSE Class 10 Chemistry Selina Solutions and other revision resources.

Study Of Acids, Bases and Salts Exercise 70

Solution 1

Solution 2

(a) (i) Hydrogen chloride HCl
(ii) Nitric acid HNO₃
(b) (i) Carbonic acid H₂CO₃
(ii) Oxalic acid (COOH)₂
(c) (i) Sulphuric acid H₂SO₄
(ii) Hydrogen chloride HCl
(d) (i) Carbonic acid H₂CO₃
(ii) Acetic acid

Solution 3

Solution 4

(a) The pH of a solution is defined as the negative logarithm (base 10) of the hydronium ion concentration present in the solution.
pH = -log₁₀ [H₃O+]
(b) The three applications of pH scale are:

It is used to determine the acidic or basic nature of the solution.
It is used to determine hydronium ion concentration present in the solution.
It is used to find out neutrality of the solution.

Solution 5

Solution 6

Solution 7

(a) Base in solution furnishes the ions:
Hydroxide ion/ oxide ion and a metallic ion.
(b) A weak alkali furnishes the ions:
Hydroxide ion and metallic ion and molecules of weak alkali./
(c) An acid in a solution furnishes the ions:
Hydronium / Hydrogen ion and a negative ion.

Solution 8

Solution 9

(a) CaO
(b) NaOH
(c) CuO
(d) Cu[(OH)₂]
(e) H₂CO₃
(f) Ferric hydroxide [Fe (OH)₃].
(g) CuO
(h) NH₃

Study Of Acids, Bases and Salts Exercise 71

Solution 10

Anhydrous hydrogen chloride is not an acid but its aqueous solution is a strong acid because anhydrous means without water and we know that the property of acidity is shown by a substance only when it is dissolved in water or its aqueous solution is prepared.

Solution 11

Solution 12

Strength of an acid measures the ease with which the acid can ionize to produce hydrogen or hydronium ions when dissolved in water. Those acids which can easily ionize to form hydrogen ions are called strong acids while those which can partially ionize to form hydrogen ions are called weak acids.
Strength of an acid depends upon many factors such as:

Molecular structure of the acid

The temperature

Properties of the solvent

Solution 13

Solution 14

Solution B with pH value 9 will give pink colour with phenolphthalein.
Concept Insight: Bases give pink colour with phenolphthalein because a base will abstract two protons from phenolphthalein and the resulting phenolphthalein ion provides pink colour to the solution.

Solution 15

Two indicators for identification of acid are methyl red and Thymol blue.

Solution 16

Solution 17

Solution 18

Solution 19

Solution 20

(i) Efflorescence: It is the phenomenon by which hydrated salts on exposure to dry air, lose their water of crystallization and crumble to powder.
(ii) Hygroscopy: It is the phenomenon by which substances absorb moisture from air, but only sufficiently so as to become wet.
(iii) Water of crystallization: It is the fixed amount of water that is present in a crystal as an integral part of its constitution. Hydrated salts are salts having water of crystallisation.

Solution 21

Deliquescence is the phenomenon by which certain salts absorb moisture from air, lose their water of crystallization and dissolve in it to form a saturated solution.
The substances which exhibit deliquescence are called deliquescent.
For example Caustic soda NaOH, Caustic potash KOH.

Solution 22

Solution 23

Solution 24

(a) Common salt gets wet during rainy season because the commercially available salt contains impurities, like magnesium chloride, which are deliquescent substances. These absorb moisture from atmosphere and make the table salt wet.
(b) (i) Na₂CO₃.10H₂O = Washing soda
(ii) MgSO₄.7H₂O = Epsom salt
(iii) CuSO₄.5H₂O = Blue vitriol
(iv) ZnSO₄.7H₂O = White vitriol

Solution 25

Reactions of SO₂:

Reactions of oxides of nitrogen:

Solution 26

(a) The word acid comes from the latin word acidus meaning 'sour'.

(b) Vinegar is the source of acetic acid.

(d) pH scale was introduced by Sorencen in 1909.

(e) Efflorescence is the phenomenon by which hydrated salts on exposure to dry air lose their water of crystallisation and crumble to powder.

Study Of Acids, Bases and Salts Exercise 72

Solution 27

(i) Citric acid

(ii) Food preservative

(iii) Violet

(iv) Calcium chloride

Solution 1996-1

(i) pH of a solution having pH 7 can be increased by adding a base to it such as NaOH.
(ii) pH can be decreased by adding an acid such as HCl to it.
If a solution changes colour of litmus from red to blue, it shows that its pH is above 7.

Solution 1996-2

Solution 1996-3

(a) Zinc sulphate = Zinc and dilute sulphuric acid
(b) Copper sulphate = Copper oxide and dilute sulphuric acid
(c) Sodium sulphate = Sodium carbonate solution and dilute sulphuric acid
(d) Lead sulphate = Lead carbonate and dilute sulphuric acid

Solution 1997-1

The term acid salt means the salt formed by partial replacement of the hydrogens present in the acid by metallic or ammonium ions.
For example: NaHCO₃

Solution 1997-2

(i) pH scale is used to express the acidic or basic nature of solution.
(ii) pH of pure water is 7 since it does not have any impurities.
(iii) (a) A soluble oxide of A will have pH less than the pH of pure water i.e. below 7.
(b) A solution of 'B' will have more pH than pure water i.e. above 7.

Solution 1997-3

(i) Water of crystallization: It is the fixed amount of water that is present in a crystal as an integral pat of its constitution. Compounds having water of crystallization are called hydrous salts.
For example: Sodium carbonate Na₂CO₃ has 10 molecules of water present as water of crystallization Na₂CO₃.10H₂O
(ii) Anhydrous: Hydrous salt on heating lose their water of crystallization, such salts are then called anhydrous.
For example: Na₂CO₃.10H₂O on losing 10 molecules of water forms Na₂CO₃.

Solution 1997-4

Study Of Acids, Bases and Salts Exercise 73

Solution 1998-1

(i) Water of cystallization.
(ii) White.
(iii) Efflorescence.
(iv) Sodium chloride.

Solution 1998-2

Those acids which ionize partially in aqueous solution and thus they contain ions as well as molecules of the acid. Organic acid such as CH₃COOH, is a weak acid.

Solution 1998-3

Solution 1998-4

The name and formula of the acid salt which gives sodium ions and sulphate ions in solution is Sodium hydrogen sulphate NaHSO₄.

Solution 1999-1

Solution 2000-1

Study Of Acids, Bases and Salts Exercise 74

Solution 2001-1

Solution 2002-1

Solution 2003-1

(i) Hydronium, positive.
(ii) Acid, metal.

Solution 2003-2

Solution 2004-1

methods for preparation:
(i) Preparation of copper(II) chloride.
Action of an acid on an oxide or carbonate
(ii) Preparation of iron(III) chloride.
Direct combination
(iii) Preparation of iron (II) chloride.
Action of an acid on a metal
(iv) Preparation of lead (ii) chloride
Precipitation (double decomposition)
(v) Preparation of sodium chloride
Neutralization of an alkali by an acid.

Study Of Acids, Bases and Salts Exercise 75

Solution 2005-1

Solution 2005-2

Positive, hydroxyl, Salt, Neutralization.

Solution 2005-3

When neutral litmus solution is added to sodium hydrogen carbonate solution, litmus solution turns red

Solution 2006-1

(a) From pink to colourless.
(b) From orange to pink.
(c) From colourless to red.

Solution 2007-1

(i) Hydronium
(ii) Hydroxide
(iii) Salt
(iv) Water
(v) Hydrogen

Solution 2007-2

Study Of Acids, Bases and Salts Exercise 76

Solution 2008-1

(i) Complex salt.
(ii) Alkali.

Solution 2009-1

Acidified potassium dichromate paper

Solution 2009-2

(i) Solution B.
(ii) Solution A.
(iii) Solution B
(iv) Solution of ammonium hydroxide NH₄OH is a weak alkali.

Solution 2009-3

Study Of Acids, Bases and Salts Exercise 77

Solution 2010-1

(i) A

(ii) A

(iii) D

Solution 2010-2

Solution 2010-3

(i)

(ii)

(iii)

(iv)

Solution 2010-4

(i) C = Dilute sulphuric acid

(ii) A = Sodium hydroxide

(iii) B = Weak acid

Solution 2011-1

When crystals of washing soda are exposed to air, it loses its water of crystallisation and the phenomenon is known as efflorescence.

Solution 2011-2

(i) (B) Neutralisation

(ii) (E) Direct synthesis

(iii) (D) Double decomposition

(iv) (A) Simple displacement

(v) (C) Decomposition by acid

Solution 2013-1

(i) Hydronium

(ii) Hydroxide

(iii) Salt

(iv) Water

(v) Hydrogen

Study Of Acids, Bases and Salts Exercise 78

Solution 2016-1

(a) When washing soda (Na₂CO₃.10H₂O) is exposed to air, it loses 9 molecules of water to form a monohydrate.

(b) It absorbs moisture from the atmosphere and becomes moist and ultimately dissolves in the absorbed water, forming a saturated solution.

Solution 2016-2

Column I

Column II

(i) P(NO₃)₂ from PbO

(ii) MgCl₂ from Mg

(iii) FeCl₃from Fe

(iv) NaNO₃ from NaOH

(v) ZnCO₃ from ZnSO₄

(A) Precipitation

(F) Simple displacement

(B) Combination

(G) Neutralisation

(H) Titration

Solution 2017-1

(a) When a metallic oxide is dissolved in water, the solution formed has a high concentration of OH⁻ ions.

Solution 2017-2

(b) (c) An alkali

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