Consider the two gaseous equilibria involving SO₂ and the corresponding equilibrium constants at 298 K

SO₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ SO₃ (g); K₁

2SO₃ (g) $\rightleftharpoons$ 2SO₂ (g) + O₂ (g); K₂

The values of the equilibrium constants are related by

• K₂ = K₁

• K₂ = K${}_1^2$

• K₂ = $\frac{1}{{\mathrm{K}}_1^2}$

• K₂ = $\frac{1}{{\mathrm{K}}_1}$

For the reaction,

A + B $\rightleftharpoons$ C + D,

the initial concentrations of A and B are equal. The equilibrium concentration of C is two times the equilibrium concentration of A. The equilibrium constant is

• 4

• $\frac{1}{4}$

• 9

• $\frac{1}{9}$

The pOH of a solution is 6.0. Its pH will be

• 6

• 8

• 0

• 14

Solubility products of Al(OH)₃ and Zn(OH)₂ are 8.5 × 10^-23 and 1.8 × 10^-4 respectively. If both Al³⁺ and Zn²⁺ ions are present in a solution, which one will be precipitated first on addition of NH₄OH?

• Al(OH)₃

• Zn(OH)₂

• Both (a) and (b)

• None of these

605.

The weakest acid among the following is

• CH₃COOH

• CH₂ClCOOH

• CHCl₂COOH

• CCl₃COOH

Nitric acid ionises slightly in HF,

$\underset{\left(\mathrm{Solvent}\right)}{{\mathrm{HNO}}_3 + \mathrm{HF} \rightleftharpoons {\mathrm{H}}_2{\mathrm{NO}}_3^{+} + {\mathrm{F}}^{-}}$ Then.

• HNO₃ and H₂NO${}_3^{+}$

• HF and F^- are bases

• HNO₃ and F^- are bases

• only HNO₃ is base

For the reaction, 2NO(g) + Cl₂(g) $\rightleftharpoons$2NOCl(g). which relation is true ?

• K_P=K_c × RT

• ${\mathrm{K}}_{\mathrm{P}}= \frac{{\mathrm{K}}_{\mathrm{c}}}{\mathrm{RT}}$

• ${\mathrm{K}}_{\mathrm{P}}= {\mathrm{K}}_{\mathrm{c}}(\mathrm{RT}{)}^2$

• ${\mathrm{K}}_{\mathrm{P}}= \frac{{\mathrm{K}}_{\mathrm{c}}}{{\left(\mathrm{RT}\right)}^2}$

If the molar solubility of X₃B₃(AlF₆)₂ at 298 K is x, the solubility product K_sp is

• 18x³

• 27x⁴

• 27x⁸

• 2916x⁸

The pH of 0.05 M solution of a strong dibasic acid is

• 0.0

• 1.0

• 0.2

• 0.5

For the equilibrium reaction,

2SO₂ (g) + O₂ (g) $\rightleftharpoons$ 2SO₃ (g) + $∆$H

the increase in temperature

• favours the formation of SO₃

• favours the decomposition of SO₃

• does not affect the equilibrium

• stops the reaction