For `10^(-4)` M BOH (weak base) ,`K_(b)=5xx10^(-5))`:

Options

A. `alpha=0.707`
B. `[OH^(-)]=5xx10^(-5)M`
C. `pH=9.85`
D. All of these

Explanation

To solve the problem step by step, we need to calculate the degree of dissociation (α), the concentration of hydroxide ions (OH⁻), and the pH of the solution for a weak base BOH with a concentration of \(10^{-4}\) M and a base dissociation constant \(K_b = 5 \times 10^{-5}\).

### Step 1: Calculate the degree of dissociation (α)

The degree of dissociation (α) can be calculated using the formula:

\[
\alpha = \sqrt{\frac{K_b}{C}}
...