The dissociation constant of two acids HA₁ and HA₂ are $3.0\times {10}^{-4}$ and $1.8\times {10}^{-5}$ respectively. The relative strengths of the acids is

1. 1:16

2. 1:4

3. 4:1

4. 16:1

0.005 M acid solution has 5 pH. The percentage ionization of acid is

1. 0.8%

2. 0.6%

3. 0.4%

4. 0.2%

100 ml of 0.015 M HCl solution is mixed with 100 ml of 0.005 M HCl. What is the pH of the resultant solution?

1. 2.5

2. 1.5

3. 2

4. 1

The solubility product of A₂X₃ is $1.08\times {10}^{-23}$. Its solubility will be

1. $1.0\times {10}^{-3} \mathrm{M}$

2. $1.0\times {10}^{-4} \mathrm{M}$

3. $1.0\times {10}^{-5} \mathrm{M}$

4. $1.0\times {10}^{-6} \mathrm{M}$

M(OH) x has ${\mathrm{K}}_{\mathrm{sp}}=4\times {10}^{-12}$ and solubility 10^-4 M, x is

1. 1

2. 2

3. 3

4. 4

The pH values of 1 M solutions of CH₃COOH (I), CH₃COONa (II), CH₃COONH₄ (III), and KOH (IV) will be in the order

1. IV>III>II>I

2. IV>II>III>I

3. I>III>II>IV

4. II>I>III>IV

The ratio of the concentration of salt and acid for preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid will be: (K_a=10^-5)

1. 1:10

2. 10:1

3. 100:1

4. 1:100

The strongest Bronsted base among the following ions is:

1. CH₃O^-

2. (CH₃)₂CHO^-

3. C₂H₅O^-

4. (CH₃)₃CO^-

The degree of ionization of water was found to be $1.8\times {10}^{-9}$. The ${\mathrm{K}}_{\mathrm{a}}$ (ionization constant) of water is

1. $1.8\times {10}^{-9}$

2. $1.8\times {10}^{-16}$

3. $1.8\times {10}^{-14}$

4. cannot be calculated

The decreasing order of the acidic nature of ${\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{I}\right), {\mathrm{H}}_3{\mathrm{PO}}_4 \left(\mathrm{II}\right), \mathrm{and} {\mathrm{HClO}}_4 \left(\mathrm{III}\right)$ is:

1. I>II>III

2. I>III>II

3. III>I>II

4. III>II>I