The pH of a solution obtained by mixing 100ml of 0.2 M CH₃COOH with 100ml of 0.2 M NaOH would be (given pKa for CH₃COOH = 4.74)

1. 4.74

2. 8.87

3. 9.10

4. 8.57

For N₂ + 3H₂ $\rightleftharpoons$2NH₃, one mole of N₂ and three moles of H₂ are at pressure of 4 atm. Equilibrium pressure is found to be 3 atm. Hence, K_p is

1.    1/(0.5)x(0.15)³               2. 1/(0.5)x(1.5)³

3. 3x3/(0.5)x(1.5)³                 4. none of the above

If carbon dioxide is 2% dissociated at equilibrium 2CO₂ (g)$\rightleftharpoons$2CO(g) + O₂(g). The mole fraction of CO₂ at equuilibrium is

1. 1.01/0.98           

2. 0.98/1.01

3. 0.01/0.98           

4. 0.098/1.01

To a 200 ml of 0.1 M weak acid HA solution 90 ml of 0.1 M solution of NaOH be added, Now, what volume of 0.1 M NaOH be added into above solution so that pH of resulting solution be 5.

[K_a(HA) = 10^-5]

1. 2 ml               

2. 20 ml

3. 10 ml             

4. 15 ml

Calculate the molar solublity of Fe(OH)₂ at a pH of 8

[K_sp of Fe(OH)₂ = 1.6 X 10^-14]

1. 0.06

2. 0.016

3. 0.01

4. 0.16

The strongest Lewis acid among the following is:

1. BBr₃

2. BCl₃

3. BF₃

4. All are same

When a solution of acetic acid was titrated with NaOH, the pH of the solution when half of the acid, neutralised was 4.2. Dissociation constant of the acid is

1. 6.31 × 10^-5

2. 3.2 × 10^-5

3. 8.7 × 10^-8

4. 6.42 × 10^-4

A 20 litre container at 400 K contains CO₂(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of CO₂ attains its maximum value, when the pressure of C02 attains its maximum value, will be

(Given that: SrCO₃(s) $\rightleftharpoons$ SrO(s) + CO₂(g), (Kp =1.6 atm))

(1) 5 L

(2) 10 L

(3) 4L

(4) 2L

The equilibrium constant of the following are

${\mathrm{N}}_2+ 3{\mathrm{H}}_2\stackrel{ }{\rightleftharpoons }2{\mathrm{NH}}_3; {\mathrm{K}}_1$
${\mathrm{N}}_2 + {\mathrm{O}}_2 \stackrel{ }{\rightleftharpoons }2\mathrm{NO}; {\mathrm{K}}_2$
${\mathrm{H}}_2 + \frac{1}{2}{\mathrm{O}}_2 \stackrel{ }{\to }{\mathrm{H}}_2\mathrm{O}; {\mathrm{K}}_3$

The equilibrium constant (K) of the reaction

$2{\mathrm{NH}}_3 + \frac{5}{2}{\mathrm{O}}_2 \stackrel{ \mathrm{K} }{\rightleftharpoons }2\mathrm{NO} + 3{\mathrm{H}}_2\mathrm{O},$ will be

(a) ${\mathrm{K}}_1\raisebox{1ex}{${\mathrm{K}}_3^3$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_2$}\right.$

(b) ${\mathrm{K}}_2\raisebox{1ex}{${\mathrm{K}}_3^3$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

(c) ${\mathrm{K}}_2\raisebox{1ex}{${\mathrm{K}}_3^{}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

(d) ${\mathrm{K}}_2^3\raisebox{1ex}{${\mathrm{K}}_3^{}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{K}}_1$}\right.$

The concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 x 10^-4 M. The solubility product of Ag₂C₂O₄ is

1. 2.42 x 10^-8

2. 2.66 x 10^-12

3. 4.5 x 10^-11

4. 5.3 x 10^-12