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

1.	Na2CO3	2.	OH-
3.	HCO3-	4.	NH3

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: 

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)