The acid ionization (hydrolysis) constant of `Zn^(2+)" is "1.0 xx 10^(-9)`
Calculate the pH of a 0.001 M solution of ZnCl2

Explanation

To calculate the pH of a 0.001 M solution of ZnCl2, we can follow these steps:

### Step 1: Identify the given data
- The acid ionization constant (hydrolysis constant) of \( Zn^{2+} \) is given as \( K_a = 1.0 \times 10^{-9} \).
- The concentration of the ZnCl2 solution is \( 0.001 \, M \).

### Step 2: Calculate the base ionization constant (\( K_b \))
We know that the relationship between the acid ionization constant (\( K_a \)) and the base ionization constant (\( K_b \)) is given by:
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