Calculate the hydrolysis constant `(K_(h))` and degree of hydrloysis `(h)` of `NH_(4)C1` in `0.1M` solution.
`K_(b) = 2.0 xx 10^(-5)`. Calculate the `[overset(Theta)OH]` ions in the solution.

Explanation

To solve the problem, we need to calculate the hydrolysis constant (K_h), the degree of hydrolysis (h), and the concentration of hydroxide ions ([OH⁻]) for a 0.1 M solution of NH₄Cl. We are given that K_b for NH₄⁺ is 2.0 × 10⁻⁵.

### Step 1: Calculate the Hydrolysis Constant (K_h)

The hydrolysis constant (K_h) can be calculated using the formula:

\[ K_h = \frac{K_w}{K_b} \]

Where:
- \( K_w \) is the ion product of water, which is \( 1.0 \times 10^{-14} \) at 25°C.
- \( K_b \) is the base dissociation constant for NH₄⁺, which is given as \( 2.0 \times 10^{-5} \).

Substituting the values:

\[ K_h = \frac{1.0 \times 10^{-14}}{2.0 \times 10^{-5}} = 5.0 \times 10^{-10} \]

### Step 2: Calculate the Degree of Hydrolysis (h)

The degree of hydrolysis (h) can be calculated using the formula:

\[ h = \sqrt{\frac{K_h}{C}} \]

Where:
- \( C \) is the concentration of the solution, which is given as 0.1 M.

Substituting the values:

\[ h = \sqrt{\frac{5.0 \times 10^{-10}}{0.1}} = \sqrt{5.0 \times 10^{-9}} = 7.07 \times 10^{-5} \]

### Step 3: Calculate the Concentration of Hydroxide Ions ([OH⁻])

The concentration of hydroxide ions can be calculated using the formula:

\[ [OH^-] = C \cdot h \]

Substituting the values:

\[ [OH^-] = 0.1 \times 7.07 \times 10^{-5} = 7.07 \times 10^{-6} \text{ M} \]

### Final Results

1. Hydrolysis constant (K_h) = \( 5.0 \times 10^{-10} \)
2. Degree of hydrolysis (h) = \( 7.07 \times 10^{-5} \)
3. Concentration of hydroxide ions ([OH⁻]) = \( 7.07 \times 10^{-6} \text{ M} \)