iCON Education - Ionic Equilibrium

2019 Q101 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The molar solubility of Cd(OH)₂ is 1.84 × 10^–5 M in water. The expected solubility of Cd(OH)₂ in a buffer solution of pH = 12 is :

A.

2.49 × 10^–10 M

B.

1.84 × 10^–9 M

C.

6.23 × 10^–11 M

D.

${{2.49} \over {1.84}} \times {10^{ - 9}}M$

Correct Answer: A

Explanation:

Cd(OH)₂(s)	⇌	Cd²⁺(aq)	+	2OH^$-$(aq)
		S		2S

$ \therefore $ K_sp[Cd(OH)₂] = 4(S)³ = 4(1.84 × 10^–5)³ [Given S = 1.84 × 10^–5]

For buffer solution of pH = 12 :
As pH = 12 so pOH = 2
$ \Rightarrow $ [OH^$-$] = 10^-2
Let the solubilty = S₁

Cd(OH)₂(s)	⇌	Cd²⁺(aq)	+	2OH^$-$(aq)
		S₁		2S₁ + 10^-2

$ \therefore $ K_sp[Cd(OH)₂] = S₁(10^-2)² = 4(1.84 × 10^–5)³
$ \Rightarrow $ S₁ = 2.49 × 10^–10 M

2019 Q102 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

What is the molar solubility of Al(OH)₃ in 0.2 M NaOH solution ? Given that, solubility product of Al(OH)₃ = 2.4 × 10^–24 :

A.

3 × 10^–22

B.

3 × 10^–19

C.

12 × 10^–21

D.

12 × 10^–22

2019 Q103 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The pH of a 0.02 M NH₄Cl solution will be :
[given K_b (NH₄OH) = 10^–5 and log 2 = 0.301]

A.

2.56

B.

5.35

C.

4.35

D.

4.65

2019 Q104 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Consider the following statements
(a) The pH of a mixture containing 400 mL of 0.1 M H₂SO₄ and 400 mL of 0.1 M NaOH will be approximately 1.3
(b) Ionic product of water is temperature dependent.
(c) A monobasic acid with Ka = 10^–5 has pH = 5. The degree of dissociation of this acid is 50 %.
(d) The Le Chatelier's principle is not applicable to common-ion effect.

The correct statements are :

A.

(a) and (b)

B.

(a), (b) and (c)

C.

(a), (b) and (d)

D.

(b) and (c)

2019 Q105 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

In an acid-base titration, 0.1 M HCl solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titraction mixture in this experiment?

JEE Main 2019 (Online) 9th April Evening Slot Chemistry - Ionic Equilibrium Question 105 English

A.

(C)

B.

(A)

C.

(B)

D.

(D)

2019 Q106 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

If solublity product of Zr₃(PO₄)₄ is denoted by K_sp and its molar solubility is denoted by S, then which of the following relation between S and K_sp is correct ?

A.

$S = {\left( {{{{K_{sp}}} \over {929}}} \right)^{1/9}}$

B.

$S = {\left( {{{{K_{sp}}} \over {6912}}} \right)^{1/7}}$

C.

$S = {\left( {{{{K_{sp}}} \over {144}}} \right)^{1/6}}$

D.

$S = {\left( {{{{K_{sp}}} \over {216}}} \right)^{1/7}}$

Correct Answer: B

Explanation:

Zr₃(PO₄)₄	⇌	3Zr⁺⁴	+	4PO₄^-3
S		3S		4S

K_sp = [Zr⁺⁴]³ [PO₄^-3]⁴

= [3S]³ [4S]⁴

= 27S³ $ \times $ 256S⁴

= 6912S⁷

$ \therefore $ $S = {\left( {{{{K_{sp}}} \over {6912}}} \right)^{1/7}}$

2019 Q107 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

If K_sp of Ag₂CO₃ is 8 $ \times $ 10^–12, the molar solubility of Ag₂CO₃ in 0.1 M AgNO₃ is -

A.

8 $ \times $ 10^–12 M

B.

8 $ \times $ 10^–10 M

C.

8 $ \times $ 10^–13 M

D.

8 $ \times $ 10^–11 M

2019 Q108 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

A mixture of 100 m mol of Ca(OH)₂ and 2 g of sodium sulphate was dissolved in water and the volume was made up to 100 mL. The mass of calcium sulphate formed and the concentration of OH^– in resulting solution, respectively, are : (Molar mass of Ca (OH)₂, Na₂SO₄ and CaSO₄ are 74, 143 and 136 g mol^–1 , respectively; K_sp of Ca(OH)₂ is 5.5 × 10^–6 )

A.

13.6g, 0.28 mol L^$-$1

B.

13.6g, 0.14 mol L^$-$1

C.

1.9g, 0.28 mol L^$-$1

D.

1.9g, 0.14 mol L^$-$1

2019 Q109 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The pH of rain water, is approximately :

A.

5.6

B.

7.5

C.

7.0

D.

6.5

2019 Q110 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

20 mL of 0.1 M H₂SO₄ solution is added to 30 mL of of 0.2 M NH₄OH solution. The pH of the resultant mixture is : [pk_b of NH₄OH = 4.7].

A.

5.2

B.

9.0

C.

5.0

D.

9.4

2018 Q111 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

An alkali is titrated against an acid with methyl orange as indicator, which of the following is a correct combination?

A.

Base	Acid	End point
Weak	Strong	Colourless to pink

B.

Base	Acid	End point
Strong	Strong	Pinkish red to yellow

C.

Base	Acid	End point
Weak	Strong	Yellow to pinkish red

D.

Base	Acid	End point
Strong	Strong	Pink to colourless

2018 Q112 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Which of the following salts is the most basic in aqueous solution?

A.

Pb(CH₃COO)₂

B.

Al(CN)₃

C.

CH₃COOK

D.

FeCl₃

2018 Q113 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

An aqueous solution contains an unknown concentration of Ba²⁺. When 50 mL of a 1 M solution of Na₂SO₄ is added, BaSO₄ just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO₄ is 1 $\times$ 10^–10. What is the original concentration of Ba²⁺?

A.

1.0 $\times$ 10^–10 M

B.

5 $\times$ 10^–9 M

C.

2 $\times$ 10^–9 M

D.

1.1 $\times$ 10^–9 M

2018 Q114 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Which of the following are Lewis acids?

A.

BCl₃ and AlCl₃

B.

PH₃ and BCl₃

C.

AlCl₃ and SiCl₄

D.

PH₃ and SiCl₄

2018 Q115 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0 $\times$ 10^–7 and that of S^2- from HS^– ions is 1.2 $\times$ 10^–13 then the concentration of S^2- ions in aqueous solution is :

A.

5 $\times$ 10^–19

B.

5 $\times$ 10^–8

C.

3 $\times$ 10^–20

D.

6 $\times$ 10^–21

2018 Q116 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Following four solutions are prepared by mixing different volumes of NaOH and HCl of different concentrations, pH of which one of them will be equal to 1 ?

A.

100 mL ${M \over {10}}$ HCl + 100 mL ${M \over {10}}$ NaOH

B.

75 mL ${M \over {5}}$ HCl + 25 mL ${M \over {5}}$ NaOH

C.

60 mL ${M \over {10}}$ HCl + 40 mL ${M \over {10}}$ NaOH

D.

55 mL ${M \over {10}}$ HCl + 45 mL ${M \over {10}}$ NaOH

2018 Q117 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The minimum volume of water required to dissolve 0.1 g lead (II) chloride to get a saturated solution (K_sp of PbCl₂ = 3.2 $ \times $ 10^-8 atomic mass of Pb = 207 u ) is :

A.

0.36 L

B.

17.98 L

C.

0.18 L

D.

1.798 L

Correct Answer: C

Explanation:

Given,

K_sp of PbCl₂ = 3.2 $ \times $10^$-$8

	PbCl₂ $\rightleftharpoons$	Pb²⁺	2Cl
Initially	1	0	0
At equilibrium	1-s	s	2s

K_sp = [s] [2s]²

$\therefore\,\,\,\,$ K_sp = 4s³

$\therefore\,\,\,\,$ 4s³ = 3.2 $ \times $ 10^$-$8

$ \Rightarrow $ $\,\,\,\,$ s³ = 8 $ \times $ 10^$-$9

$ \Rightarrow $ $\,\,\,\,$ s = 2 $ \times $ 10 ^$-$3 M

Solubility = ${{no.\,\,of\,moles\,\,of\,\,pbc{l_2}\,} \over {volume\,(in\,\,litre)}}$

$\therefore\,\,\,\,$ 2 $ \times $ 10^$-$3 = ${{0.1} \over {278}}$ $ \times $ ${1 \over V}$

$ \Rightarrow $ $\,\,\,\,$ V = ${{0.1} \over {278}}$ $ \times $ ${{{{10}^3}} \over 2}$ = 0.18 L

2018 Q118 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Which of the following is a Lewis acid?

A.

PH₃

B.

B(CH₃)₃

C.

NaH

D.

NF₃

2017 Q119 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

50 mL of 0.2 M ammonia solution is treated with 25 mL of 0.2 M HCl. If pK_b of ammonia solution is 4.75, the pH of the mixture will be :

A.

3.75

B.

4.75

C.

8.25

D.

9.25

2017 Q120 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Additin of sodium hydroxide solution to a weak acid (HA)results in a buffer of pH 6. If ionition constant of HA is 10^$-$5, the ratio of salt to acid concentration in the buffer solution will be :

A.

4 : 5

B.

1 : 10

C.

10 : 1

D.

5 : 4

2017 Q121 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

pK_a of a weak acid (HA) and pK_b of a weak base (BOH) are 3.2 and 3.4, respectively. The pH of their salt (AB) solution is :

A.

6.9

B.

7.0

C.

1.0

D.

7.2

2013 Q122 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

How many litres of water must be added to 1 litre of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?

A.

0.1 L

B.

0.9 L

C.

2.0 L

D.

9.0 L

2012 Q123 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, K_a of this acid is :

A.

3 $\times$ 10^–1

B.

1 $\times$ 10^–3

C.

1 $\times$ 10^–5

D.

1 $\times$ 10^–7

2010 Q124 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Three reactions involving $H_2PO_4^−$ are given below :

(i) H₃PO₄ + H₂O $\to$ H₃O⁺ + $H_2PO_4^−$

(ii) $H_2PO_4^−$ + H₂O $\to$ $HPO_4^{2−}$ + H₃O⁺

(iii) $H_2PO_4^−$ + OH^- $\to$H₃PO₄ + O^2-

In which of the above does $H_2PO_4^−$ act as an acid?

A.

(ii) only

B.

(i) and (ii)

C.

(iii) only

D.

(i) only

Correct Answer: A

Explanation:

To determine in which reactions $ H_2PO_4^- $ acts as an acid, we need to understand the Bronsted-Lowry concept of acids and bases. According to this concept, an acid is a substance that donates a proton (H⁺) to another substance, while a base is a substance that accepts a proton.

Let's analyze each reaction :

1. $ H_3PO_4 + H_2O \to H_3O^+ + H_2PO_4^- $
- In this reaction, $ H_3PO_4 $ is donating a proton to $ H_2O $, forming $ H_3O^+ $ and $ H_2PO_4^- $.
- $ H_2PO_4^- $ is the product of this reaction and is not acting as an acid here.

2. $ H_2PO_4^- + H_2O \to HPO_4^{2−} + H_3O^+ $
- In this reaction, $ H_2PO_4^- $ donates a proton to $ H_2O $, resulting in $ HPO_4^{2−} $ and $ H_3O^+ $.
- $ H_2PO_4^- $ is acting as an acid in this reaction.
3. $ H_2PO_4^- + OH^- \to H_3PO_4 + O^{2-} $
- This reaction is not correctly balanced and does not follow standard chemical reaction rules. The product $ O^{2-} $ is highly unlikely in aqueous solutions due to its reactivity.
- A more correct reaction would be $ H_2PO_4^- + OH^- \to HPO_4^{2−} + H_2O $. In this corrected reaction, $ H_2PO_4^- $ is donating a proton to $ OH^- $, which makes it an acid.

Given the information, the correct option is :

Option A : (ii) only

This is because in reaction (ii), $ H_2PO_4^- $ is clearly acting as an acid by donating a proton to water. In reaction (i), $ H_2PO_4^- $ is not acting as an acid but rather is formed as a product. Reaction (iii) as written is chemically incorrect, but even in a corrected form, it would show $ H_2PO_4^- $ acting as an acid.

2010 Q125 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Solubility product of silver bromide is 5.0 $\times$ 10^–13. The quantity of potassium bromide (molar mass taken as 120g of mol^–1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is :

A.

1.2 $\times$ 10^–10 g

B.

1.2 $\times$ 10^–9 g

C.

6.2 $\times$ 10^–5 g

D.

5.0 $\times$ 10^–8 g

2010 Q126 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

At 25°C, the solubility product of Mg(OH)₂ is 1.0 $\times$ 10^–11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

A.

9

B.

10

C.

11

D.

8

2009 Q127 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Solid Ba(NO₃)₂ is gradually dissolved in a 1.0 $\times$ 10^-4 M Na₂CO₃ solution. At what concentration of Ba²⁺ will a precipitate begin to form ?
(K_sp for BaCO₃ = 5.1 $\times$ 10⁻⁹ )

A.

5.1 $\times$ 10^-5 M

B.

8.1 $\times$ 10^-8 M

C.

8.1 $\times$ 10^-7 M

D.

4.1 $\times$ 10^-5 M

2008 Q128 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The pK_a of a weak acid, HA, is 4.80. The pK_b of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be

A.

9.58

B.

4.79

C.

7.01

D.

9.22

2008 Q129 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Four species are listed below
i. $HCO_3^−$
ii. $H_3O^+$
iii. $HSO_4^−$
iv. $HSO_3F$
Which one of the following is the correct sequence of their acid strength?

A.

iv < ii < iii < I

B.

ii < iii < i < iv

C.

i < iii < ii < iv

D.

iii < i < iv < ii

2007 Q130 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The pK_a of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is :

A.

7.0

B.

4.5

C.

2.5

D.

9.5

2007 Q131 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The first and second dissociation constants of an acid H₂A are 1.0 $\times$ 10⁻⁵ and 5.0 $\times$ 10⁻¹⁰ respectively. The overall dissociation constant of the acid will be :

A.

5.0 $\times$ 10⁻⁵

B.

5.0 $\times$ 10¹⁵

C.

5.0 $\times$ 10⁻¹⁵

D.

5.0 $\times$ 10⁵

2007 Q132 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

In a sautrated solution of the sparingly soluble strong electrolyte AgIO₃ (Molecular mass = 283) the equilibrium which sets in is
AgIO_3(s) $\leftrightharpoons$ Ag⁺(aq) + $IO_3^-$
If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 $\times$10⁻⁸, what is the mass of AgIO₃ contained in 100 ml of its saturated solution?

A.

28.3 × 10⁻² g

B.

2.83 × 10⁻³ g

C.

1.0 × 10⁻⁷ g

D.

1.0 × 10⁻⁴ g

2005 Q133 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

What is the conjugate base of OH^-?

A.

O₂

B.

H₂O

C.

O^-

D.

O^-2

2005 Q134 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The solubility product of a salt having general formula MX₂, in water is: 4 $\times$ 10^-12 . The concentration of M²⁺ ions in the aqueous solution of the salt is :

A.

2.0 $\times$ 10^-6 M

B.

4.0 $\times$ 10^-10 M

C.

1.0 $\times$ 10^-4 M

D.

1.6 $\times$ 10^-4 M

2005 Q135 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :

A.

3.98 $\times$ 10^-6

B.

3.68 $\times$ 10^-6

C.

3.88 $\times$ 10⁶

D.

3.98 $\times$ 10⁸

2004 Q136 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The molar solubility (in ol L^-1) of a sparingly soluble salt MX₄ is "s". The corresponding solubility product is K_sp. 's' is given in term of K_sp by the relation :

A.

s = (256 K_sp)^1/5

B.

s = (128 K_sp)^1/4

C.

s = ( K_sp / 128)^1/4

D.

s = (K_sp / 256)^1/5

2004 Q137 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The conjugate base of H₂PO₄^- is :

A.

$PO_4^{3-}$

B.

$HPO_4^{2-}$

C.

H₃PO₄

D.

P₂O₅

2003 Q138 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Which one of the following statements is not true?

A.

pH + pOH = 14 for all aqueous solutions

B.

The pH of 1 $\times$ 10^-8 M HCl is 8

C.

96,500 coulombs of electricity when passed through a CuSO₄ solution deposits 1 gram equivalent of copper at the cathode

D.

The conjugate base of $H_2PO_4^-$ is $HPO_4^{2-}$

2003 Q139 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

The solubility in water of a sparingly soluble salt AB₂ is 1.0 $\times$ 10^-5 mol L^-1. Its solubility product number will be :

A.

4 $\times$ 10^-10

B.

1 $\times$ 10^-15

C.

1 $\times$ 10^-10

D.

4 $\times$ 10^-15

2003 Q140 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

When rain is accompanied by a thunderstorm, the collected rain water will have a pH value :

A.

slightly higher than that when the thunderstorm is not there

B.

uninfluenced by occurence of thunderstorm

C.

which depends on the amount of dust in air

D.

slightly lower than that of rain water without thunderstorm

2002 Q141 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Species acting as both Bronsted acid and base is :

A.

(HSO₄)^-1

B.

Na₂CO₃

C.

NH₃

D.

OH^-1

2002 Q142 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

Let the solubility of an aqueous solution of Mg(OH)₂ be x then its K_sp is :

A.

4x³

B.

108x⁵

C.

27x⁴

D.

9x

2002 Q143 JEE Mains MCQ

iCON Education HYD, 79930 92826, 73309 72826 14 Mar 2026

1 M NaCL and 1 M HCL are present in an aqueous solution. The solution is

A.

not a buffer solution with pH < 7

B.

not a buffer solution with pH > 7

C.

a buffer solution with pH < 7

D.

a buffer solution with pH > 7

Chemistry Chapters

Ionic Equilibrium

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