For the reaction,

H₂ (g) + I₂ (g) $\rightleftharpoons$ 2HI (g),

the equilibrium constants expressed in terms of concentrations K_c and in terms of partial pressures K_p, are related as:

• K_p = K_c (RT)²

• K_p = K_c(RT)^-2

• K_p = K_c

• K_c = K_p(RT)

Which of the following pairs are correctly matched?

1. Haber process	Manufacture of ammonia
2. Leblanc process	Manufacture of sulphuric acid
3. Birkeland-Eyde process	Manufacture of nitric acid
4. Solvay process	Manufacture of sodium carbonate

Select the correct answer using the codes given below-

• 1, 3 and 4

• 2, 3 and 4

• 1, 2, 3 and 4

• 1, 2 and 4

Which of the following will favour the reverse reaction in a chemical equilibrium ?

• Increasing the concentration of the reactants

• Removal of at least one of the products at regular intervals

• Increasing the concentration of one or more of the products

• Increasing the pressure

K_p and K_c are related as :

• K_p = K_c(RT)^Δn

• K_p + K_c = (RT)^Δn

• K_c= K_p

• K_p .K_c= (RT)^Δn

100 mL of 0.01 M solution of NaOH is diluted to 1 dm³. What is the pH of the diluted solution?

• 12

• 11

• 2

• 3

Relation between hydrolysis constant and dissociation constant are given. Which is the correct formula for MgCl₂ ?

• K_h = $\frac{{\mathrm{K}}_{\mathrm{w}}}{{\mathrm{K}}_{\mathrm{a}}}$

• K_h = $\frac{{\mathrm{K}}_{\mathrm{w}}}{{\mathrm{K}}_{\mathrm{b}}}$

• K_h = $\frac{{\mathrm{K}}_{\mathrm{w}}}{{\mathrm{K}}_{\mathrm{a} }\times {\mathrm{K}}_{\mathrm{b}}}$

• K_w = $\frac{{\mathrm{K}}_{\mathrm{h}}}{{\mathrm{K}}_{\mathrm{b}}}$

Calculate pOH of 0.001 M NH₄OH when it is 1% dissociated in the solution.

• 5

• 2.96

• 9.04

• 11.04

178.

The values of dissociation constant of bases are given below. Which is the weakest base?

• 1.8 × 10^-5

• 4.8 × 10^-10

• 7.2 × 10^-11

• 7.07 × 10^-7

The pH of millimolar HCl is

• 1

• 3

• 2

• 4

0.5 M ammonium benzoate is hydrolysed to 0.25 percent, hence, its hydrolysis constant is

• 2.5 x 10^-5

• 1.5 x 10^-4

• 3.125 x 10^-6

• 6.25 x 10^-6