Ionization constant of acetic acid is $1.8\times {10}^{-5}$. The concentration of H⁺ ions in 0.1 M solution is

1. $1.8\times {10}^{-3} \mathrm{M}$

2. $2.8\times {10}^{-3} \mathrm{M}$

3. $1.3\times {10}^{-3} \mathrm{M}$

4. $1.34\times {10}^{-4} \mathrm{M}$

The dissociation constant of a weak acid is $4.9\times {10}^{-8},$ its percentage ionization at 0.1 M is

1. 0.07%

2. 0.007%

3. 0.7%

4. 0.0007%

The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation?

1. 1%

2. 10%

3. 50%

4. 25%

75 ml of 0.2 M HCl is mixed with 25 ml of 1M HCl. To this solution, 300 ml of distilled water is added. What is the pH of the resultant solution?

1. 1

2. 2

3. 4

4. 0.2

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