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Previous year question hub

Ionic Equilibrum - Physical Chemistry - Chemistry Previous Year Questions

Practice Ionic Equilibrum - Physical Chemistry - Chemistry previous year questions organised from real papers, with year-wise coverage and clear topic navigation.

9Papers
8Years
24Questions
1Topics

Ionic Equilibrum question pattern

Every graph below is calculated only from this selection.

Questions by year

Year-wise coverage for Ionic Equilibrum. Each bar uses a separate theme-derived color.

Difficulty distribution

How the classified questions are distributed by difficulty.

Not classified 24 100%

Question type distribution

MCQ, numerical, multiple-select and other formats found in these papers.

Multiple Choices 24 100%

Subject weightage

Top subjects by unique question coverage.

Chemistry
24 Qs

Most asked topics

Top topics across the included previous year papers.

Physical Chemistry
24 Qs

Subtopic coverage

Top subtopics inside this exact selection.

Ionic Equilibrum
24 Qs

Paper coverage

Question coverage for the most populated papers. Every active PYP paper remains listed below.

WB JEE 2025
4 Qs
VITEEE 2025
1 Qs
WB JEE 2024
7 Qs
WB JEE 2023
2 Qs
WB JEE 2021
3 Qs
WB JEE 2020
1 Qs
WB JEE 2019
1 Qs
WB JEE 2017
3 Qs
WB JEE 2016
2 Qs

Included previous year papers

Newest papers appear first. Sort by year, question coverage or name.

PaperYear / sessionQuestions in this viewOpen
VITEEE 202520251View paper
WB JEE 202520254View paper
WB JEE 202420247View paper
WB JEE 202320232View paper
WB JEE 202120213View paper
WB JEE 202020201View paper
WB JEE 201920191View paper
WB JEE 201720173View paper
WB JEE 201620162View paper

All Ionic Equilibrum previous year questions

Practice every matching question in batches of 20, with every available option.

1
2016 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2016
The molar solubility (in mol L\(-\)1) of a sparingly soluble salt MX4 is 'S'. The corresponding solubility product is Ksp. S in terms of 'Ksp' is given by the relation
A
\(S = {\left( {{{{K_{sp}}} \over {128}}} \right)^{1/4}}\)
B
\(S = {\left( {{{{K_{sp}}} \over {256}}} \right)^{1/5}}\)
C
\(S = {(256{K_{sp}})^{1/5}}\)
D
\(S = {(128{K_{sp}})^{1/4}}\)
Open complete paper
2
2016 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2016
In which of the following mixed aqueous solutions, pH = pKa at equilibrium?

1. 100 mL of 0.1 M CH3COOH + 100 mL of 0.1 MCH3COONa

(2) 100 mL of 0.1 MCH3COOH + 50 mL of 0.1 M NaOH

(3) 100 mL of 0.1 M CH3COOH + 100 mL of 0.1 M NaOH

(4) 100 mL of 0.1 MCH3COOH + 100 mL of 0.1 MNH3
A
(1) is correct
B
(2) is correct
C
(3) is correct
D
Both (1) and (2) are correct
Open complete paper
3
2017 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2017
Dissolving NaCN in de-ionised water will result in a solution having
A
pH < 7
B
pH = 7
C
pOH = 7
D
pH > 7
Open complete paper
4
2017 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2017
PbCl2 is insoluble in cold water. Addition of HCl increases its solubility due to
A
formation of soluble complex anions like [PbCl3]\(-\)
B
oxidation of Pb(II) to Pb(IV)
C
formation of [Pb(H2O)6]2+
D
formation of polymeric lead complexes
Open complete paper
5
2017 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2017
Of the following compounds, which one of the strongest Bronsted acid in a aqueous solution?
A
HClO3
B
HClO2
C
HOCl
D
HOBr
Open complete paper
6
2019 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2019
Which of the following mixtures will have the lowest pH at 298 K?
A
10 mL 0.05 N CH3COOH + 5 mL 0.1 N NH4OH
B
5 mL 0.2 N NH4Cl + 5 mL 0.2 N NH4OH
C
5 mL 0.1 N CH3COOH + 10 mL 0.05 N CH3COONa
D
5 mL 0.1 N CH3COOH + 5 mL 0.1 N NaOH
Open complete paper
7
2020 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2020
A solution is saturated with SrCO3 and SrF2. The \([CO_3^{2 - }]\) is found to be 1.2 \(\times\) 10-3 M. The concentration of F- in the solution would be

Given : Ksp(SrCO3) = 7.0 \(\times\) 10-10,

Ksp(SrF2) = 7.9 \(\times\) 10-10
A
\(3.7 \times {10^{ - 6}}\) M
B
\(3.2 \times {10^{ - 3}}\) M
C
\(5.1 \times {10^{ - 7}}\) M
D
\(3.7 \times {10^{ - 2}}\) M
Open complete paper
8
2021 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2021
A saturated solution of BaSO4 at 25\(^\circ\)C is 4 \(\times\) 10\(-\)5 M. The solubility of BaSO4 in 0.1 M Na2SO4 at this temperature will be
A
1.6 \(\times\) 10\(-\)9 M
B
1.6 \(\times\) 10\(-\)8 M
C
4 \(\times\) 10\(-\)6 M
D
4 \(\times\) 10\(-\)4 M
Open complete paper
9
2021 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2021
Aqueous solution of HNO3, KOH, CH3COOH and CH3COONa of identical concentration are provided. The pair(s) of solutions which form a buffer upon mixing is (are)
A
HNO3 and CH3COOH
B
KOH and CH3COONa
C
HNO3 and CH3COONa
D
CH3COOH and CH3COONa
Open complete paper
10
2021 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2021
Solubility products (Ksp) of the salts of types MX, MX2 and M3X at temperature T are 4.0 \(\times\) 10\(-\)8, 3.2 \(\times\) 10\(-\)14 and 2.7 \(\times\) 10\(-\)15 respectively. Solubilities (in mol dm\(-\)3) of the salts at temperature T are in the order.
A
MX > MX2 > M3X
B
M3X > MX2 > MX
C
MX2 > M3X > MX
D
MX > M3X > MX2
Open complete paper
11
2023 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2023

At STP, the dissociation reaction of water is \(\mathrm{H_2O\rightleftharpoons H^+~(aq.)+OH^-~(aq.)}\), and the pH of water is 7.0. The change of standard free energy (\(\Delta\)G\(^\circ\)) for the above dissociation process is given by

A
20301 cal/mol
B
19091 cal/mol
C
20096 cal/mol
D
21301 cal/mol
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12
2023 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2023

Which of the following mixtures act(s) as buffer solution?

A
NaOH + CH\(_3\)COOH (1 : 1 mole ratio)
B
NH\(_4\)OH + HCl (2 : 1 mole ratio)
C
CH\(_3\)COOH + NaOH (2 : 1 mole ratio)
D
CH\(_3\)COOH + NaOH (1 : 2 mole ratio)
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13
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

At 25\(^\circ\)C, the ionic product of water is 10\(^{-14}\). The free energy change for the self-ionization of water in kCal mol\(^{-1}\) is close to

A
20.5
B
14.0
C
19.1
D
25.3
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14
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

Correct solubility order of \(\mathrm{AgF}, \mathrm{AgCl}, \mathrm{AgBr}, \mathrm{AgI}\) in water is

A
\(\mathrm{AgF}<\mathrm{AgCl}>\mathrm{AgBr}>\mathrm{AgI}\)
B
\(\mathrm{AgI}<\mathrm{AgBr}<\mathrm{AgCl}<\mathrm{AgF}\)
C
\(\mathrm{AgF}<\mathrm{AgI}<\mathrm{AgBr}<\mathrm{AgCl}\)
D
\(\mathrm{AgCl}>\mathrm{AgBr}>\mathrm{AgF}>\mathrm{AgI}\)
Open complete paper
15
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

What will be the change in acidity if

(i) \(\mathrm{CuSO}_4\) is added in saturated \((\mathrm{NH}_4)_2 \mathrm{SO}_4\) solution

(ii) \(\mathrm{SbF}_5\) is added in anhydrous \(\mathrm{HF}\)

A
increase, increase
B
decrease, decrease
C
increase, decrease
D
decrease, increase
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16
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

Equal volumes of aqueous solution of \(0.1(\mathrm{M}) \mathrm{HCl}\) and \(0.2(\mathrm{M}) \mathrm{H}_2 \mathrm{SO}_4\) are mixed. The concentration of \(\mathrm{H}^{+}\) ions in the resulting solution is

A
0.15 (M)
B
0.30 (M)
C
0.10 (M)
D
0.25 (M)
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17
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

Number of moles of ions produced by complete dissociation of one mole of Mohr's salt in water is

A
3
B
4
C
5
D
6
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18
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

\(\mathrm{pH}\) of \(10^{-8}(\mathrm{M}) \mathrm{~HCl}\) solution is

A
8
B
greater than 7, less than 8
C
greater than 8
D
greater than 6, less than 7
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19
2024 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2024

The specific conductance \((\mathrm{k})\) of \(0.02(\mathrm{M})\) aqueous acetic acid solution at \(298 \mathrm{~K}\) is \(1.65 \times 10^{-4} \mathrm{~S} \mathrm{~cm}^{-1}\). The degree of dissociation of acetic acid is

$$[\lambda_{\mathrm{O}^{+}}+=349.1 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1} \text { and } \lambda_{{ }^{\circ} \mathrm{CH}_3 \mathrm{COO}^{-}}=40.9 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}]$$

A
0.021
B
0.21
C
0.012
D
0.12
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20
2025 · Chemistry · Physical Chemistry · Ionic Equilibrum
WB JEE 2025

Equal volume of two solutions $A$ and $B$ of a strong acid having $\mathrm{pH}=6.0$ and $\mathrm{pH}=4.0$ respectively are mixed together to form a new solution. The pH of the new solution will be in the range

A
between 5 and 6
B
between 6 and 7
C
between 4 and 5
D
between 3 and 4
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Showing 20 of 24 questions