What is the solubility of `MgF_2` in a buffer solution containing 0.45 M `CH_3COOH ` and 0.20 M `CH_3COONa? K_(sp) (MgF_2) = 6.5 xx 10^(-9), K (HF) = 6.8 xx 10^(-4), K (CH_3COOH) = 1.7 xx 10^(-5)`

Explanation

To find the solubility of \( \text{MgF}_2 \) in a buffer solution containing \( 0.45 \, \text{M} \, \text{CH}_3\text{COOH} \) and \( 0.20 \, \text{M} \, \text{CH}_3\text{COONa} \), we will follow these steps:

### Step 1: Calculate the pH of the buffer solution
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:

\[ \text{pH} = \text{pK}_a + \log \left( \frac{[\text{Salt}]}{[\text{Acid}]} \right) \]
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