When 0.1 mole of `NH_(3)` is dissolved in water to make 1.0 L of solution, the `[OH^(-)]`of solution is `1.30xx10^(-3)M.` Calculate `K_(b)` for ` NH_(3).`

Explanation

To calculate the base dissociation constant \( K_b \) for ammonia (\( NH_3 \)), we will follow these steps:

### Step 1: Write the equilibrium reaction
When ammonia dissolves in water, it establishes an equilibrium with water as follows:

\[ NH_3 (aq) + H_2O (l) \rightleftharpoons NH_4^+ (aq) + OH^- (aq) \]
...