Calculate `[OH^(-)]and %` dissociation of 0.01 M solution of ammonium hydroxide solution. The ionization constant for
`NH_(4)OH(K_(b))=1.8xx10^(-5)`

Explanation

To solve the problem of calculating the hydroxide ion concentration \([OH^-]\) and the percentage dissociation of a 0.01 M solution of ammonium hydroxide \((NH_4OH)\) with a given ionization constant \(K_b = 1.8 \times 10^{-5}\), we can follow these steps:

### Step 1: Write the dissociation equation
The dissociation of ammonium hydroxide can be represented as:
\[ NH_4OH \rightleftharpoons NH_4^+ + OH^- \]

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