A solution has hydrogen ion concentration 0.0005 M, its pOH is

1. 8.2798

2. 10.6990

3. 12.7854

4. 13.3344

 

At 25°C, the pH of a solution containing 0.10 M sodium acetate and 0.03 M acetic acid will be:

[pK_a value of ${\mathrm{CH}}_3\mathrm{COOH}=4.57$]

1. 3.24

2. 4.59

3. 5.09

4. 6.67

Ionization constant of acetic acid(\(\mathrm{CH}_3 \mathrm{COOH}\)) 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. $1.34\times {10}^{-4} \mathrm{M}$

What is the ionization percentage for a weak acid with a dissociation constant of \(4.9×10^{−8}\) at 0.1 M concentration?

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. $1.0\times {10}^{-6} \mathrm{M}$