The equilibrium constant Kp for the following reaction is:

${{\mathrm{MgCO}}_3}_{\left(\mathrm{s}\right)}\rightleftharpoons {\mathrm{MgO}}_{\left(\mathrm{s}\right)}+{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$

1. $\mathrm{Kp }= {\mathrm{P}}_{{\mathrm{CO}}_2}$

2. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_2}\times \frac{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

3. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{CO}}_2}+{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

4. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}$

The correct relation between dissociation constants of a di-basic acid is:

1. $K{a}_1=K{a}_2$

2. $K{a}_1>K{a}_2$

3. $K{a}_1<K{a}_2$

4. $K{a}_1=\frac{1}{K{a}_2}$

For any reversible reaction, if we increase the concentration of the reactants, the effect on equilibrium constant will:
1. Depend on the amount of concentration
2. Remain unchanged
3. Decrease
4. Increase

Conjugate acid of NH₂^– is:

1. NH₄OH

2. NH₄⁺

3. \(NH_{2}^{-}\)

4. NH₃

Incorrect statement about pH and H⁺ is: 

$\mathrm{If\; A}$ $+$ $B$ $\leftrightharpoons$ $C$ $+$ $D$ $Cons\tan t$ $=$ $K_1$
$E$ $+$ $F$ $\rightleftharpoons$ $G$ $+$ $H$ $Cons\tan t$ $=$ $K_2$

then C + D + E + F ⇒ product. The constant of reaction will be:

1.  $\frac{K_1}{K_2}$

2.  $\frac{K_2}{K1}$

3. $K_1{K}_2$

4. None of these 

The fertilizer which makes the soil acidic is:

1. ${\left(N{H}_4\right)}_{2}S{O}_4$

2.  Super phosphate of lime .

3. $C{H}_{3}COONa$

4. $Ca{\left(N{O}_3\right)}_2$

Among the following examples, the species that behave(s) as a Lewis acid is/are: 
\(\mathrm{BF}_3, \mathrm{SnCl}_2, \mathrm{SnCl}_4\)

1. Stannous chloride, Stannic chloride
2. $B{F}_3$, Stannous chloride
3. Only $B{F}_3$
4. $B{F}_3$, Stannous chloride, Stannic chloride

4 gm of NaOH is dissolved in 1000 ml of water. The ${\mathrm{H}}^{+}$ ion concentration will be:

The solubility product of a sparingly soluble salt AX₂ is 3.2 ×10^–11. Its solubility (in moles/litre) is:

1. 3.1×10^–4

2. 2 × 10^–4

3. 4 × 10^–4

4. 5.6 × 10^–6