For the reaction, A(g) + 2B(g) ⇌ 3C, K_c = 10². If at equilibrium one mole of A is added and 1 mole of C is removed then, the value of K_c will be: 

1.	102	2.	103
3.	104	4.	10

Which of the following species can act as both Bronsted acid and Bronsted base in an aqueous solution?

Given that the ionic product of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ is 2 × ${10}^{-\mathrm{15 }}$. The solubility of $\mathrm{Ni}{\left(\mathrm{OH}\right)}_2$ in 0.1 M NaOH is ;
1. 2 × ${10}^{-8}$ M

Reaction quotient for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by , $\mathrm{Q}$ $=$ $\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ .The reaction will proceed from right to left if K_c value is:

An aqueous solution of NaOH has a concentration of 0.01 mol/L.
Calculate the pH of the NaOH solution at 25 °C.

Given the ionic product of water is K_w = [H⁺] [OH^–] = 10^–14 mol²/L² (at 25 °C)
1.  11

2.  7

3.  14

4.  12

The minimum volume of water required to dissolve 1g of calcium sulphate at 298 K is

(For CaSO₄ , K_sp is 9.1 × 10^–6)

1. 1.22 L

2. 0.69 L

3. 2.44 L

4. 1.87 L

If a weak base has the dissociation constant, $K_b$, then the value of the dissociation constant, $K_a$, of its conjugate acid is given by:

1. $1/K_{b }$

2. $K_w/K_{b }$

3. $K_b/K_{w }$

4. $1_{}/K_{w }$

When equal volumes of the following solutions are mixed, in which case will AgCl (K_sp = 1.8×10^–10) precipitate?

1. 10^–4 M Ag⁺ and 10^–4 M Cl^–

2. 10^–5 M Ag⁺ and 10^–5 M Cl^–

3. 10^–6 M Ag⁺ and 10^–6 M Cl^–

4. 10^–10 M Ag⁺ and 10^–10 M Cl^–

Which of the following reactions satisfies the condition \(K_p>K_c \text { ? }\)

1. H₂(g) + I₂(g) → 2HI(g)

2. N₂(g) + 3H₂(g) → 2NH₃(g)

3. 2SO₃(g) → 2SO₂(g) + O₂(g)

4. PCl₃(g) + Cl₂(g) → PCl₅(g)