Given the following two reactions:
     A + B ⇌ C + D, with rate constant K₁
     E + F ⇌ G + H, with rate constant K₂

If C + D + E + F produces a product, what is the rate constant for this reaction?

Which of the following fertilizers is responsible for making the soil acidic?

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:

A compound BA₂ has \(K_{sp} = 4\times 10^{-12}\)$.$ Solubility of this compound will be:

The equilibrium constant Kp for the following reaction is:
\(\mathrm{MgCO}_{3(\mathrm{~s})} \rightleftharpoons \mathrm{MgO}_{(\mathrm{s})}+\mathrm{CO}_{2(\mathrm{~g})}\)
1. \(\mathrm{K_P} =\mathrm{P}_{\mathrm{CO}_2}\)
2. \(\mathrm{K_P} =\mathrm{P}_{\mathrm{CO}_2} \times \frac{\mathrm{P}_{\mathrm{CO}_2 \times \mathrm{P}_{\mathrm{MgO}^{\mathrm{}}}}}{\mathrm{P}_{\mathrm{MgCO}_3}}\)
3. \(\mathrm{K_P} =\frac{\mathrm{P}_{\mathrm{CO}_2}+\mathrm{P}_{\mathrm{MgO}^{\mathrm{}}}}{\mathrm{P}_{\mathrm{MgCO}_3}}\)
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. $K{a}_1=\frac{1}{K{a}_2}$

What happens to the equilibrium constant of a reversible reaction
if the concentration of reactants is increased?

1. It depends on the amount of concentration
2. It remains unchanged
3. It decrease
4. It increase

Conjugate acid of NH₂^– is:

1. NH₄OH

2. NH₄⁺

3. \(NH_{2}^{-}\)

4. NH₃

Incorrect statement about pH and H⁺ is: