Find the degree of dissociation (α) of a 0.1 M weak monoprotic acid HA if the pH of its solution is 3.

1. 1.0%

2. 10%

3. 50%

4. 25%

Find the pH of the solution obtained by mixing 75 mL of 0.2 M HCl with 25 mL of 1.0 M HCl
and then adding 300 mL of distilled water.

1. 1.0

2. 2.0

3. 4.0

4. 0.2

The dissociation constants 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

Find the percentage ionization of a weak acid in a 0.005 M solution that has a pH of 5.

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

Find the solubility of A₂X₃ given that its solubility product  is $1.08\times {10}^{-23}$.

1. $1.0\times {10}^{-3}<mspace\; width="1em"></mspace>\mathrm{M}$

2. $1.0\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{M}$

3. $1.0\times {10}^{-5}<mspace\; width="1em"></mspace>\mathrm{M}$

4. $1.0\times {10}^{-6}<mspace\; width="1em"></mspace>\mathrm{M}$

What is the value of x for a hydroxide M(OH)_x if its solubility is  10-⁴, and its K_{sp} = 4 x 10^-12?

1. 1

2. 2

3. 3

4. 4

Given are 1 M solutions of the following:

The pH values of of the above will be in the order:

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^-