WB JEE 2023 | Ionic Equilibrium Question 1 | Chemistry

WB JEE 2023

MCQ (Single Correct Answer)

-0.25

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

20301 cal/mol

19091 cal/mol

20096 cal/mol

21301 cal/mol

WB JEE 2021

MCQ (Single Correct Answer)

-0.25

Solubility products (K_sp) 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.

MX > MX₂ > M₃X

M₃X > MX₂ > MX

MX₂ > M₃X > MX

MX > M₃X > MX₂

WB JEE 2021

MCQ (Single Correct Answer)

-0.25

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

1.6 $$\times$$ 10^$$-$$9 M

1.6 $$\times$$ 10^$$-$$8 M

4 $$\times$$ 10^$$-$$6 M

4 $$\times$$ 10^$$-$$4 M

WB JEE 2020

MCQ (Single Correct Answer)

-0.5

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 : K_sp(SrCO₃) = 7.0 $$ \times $$ 10^-10,

K_sp(SrF₂) = 7.9 $$ \times $$ 10^-10

$$3.7 \times {10^{ - 6}}$$ M

$$3.2 \times {10^{ - 3}}$$ M

$$5.1 \times {10^{ - 7}}$$ M

$$3.7 \times {10^{ - 2}}$$ M

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