Conjugate acid of NH₂^– is:

1. NH₄OH

2. NH₄⁺

3. \(NH_{2}^{-}\)

4. NH₃

Incorrect statement about pH and H⁺ is: 

At 25 ºC, the dissociation constant of a base, BOH, is 1.0 × 10^–12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:

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?

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

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

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the ratio of the concentrations of the conjugate acid (\(HIn\)) and base (\(In^–\)) forms of the indicator, as per the expression:

1. $\log \frac{\left[\mathrm{HIn}\right]}{\left[{\mathrm{In}}^{-}\right]}={\mathrm{pK}}_{\mathrm{In}}-\mathrm{pH}$

2. $\log \frac{\left[\mathrm{HIn}\right]}{\left[{\mathrm{In}}^{-}\right]}=\mathrm{pH}-{\mathrm{pK}}_{\mathrm{In}}$

3. $\log \frac{\left[{\mathrm{In}}^{-}\right]}{\left[\mathrm{HIn}\right]}=\; pH\; +\hspace{0.17em}{\mathrm{pK}}_{\mathrm{In<mspace\; width="1em"></mspace>}}$

4. None of the above