Calcuate the `pH of 0.1 Mna_(3)A` of solution (salt of tribasic acid `H_(3)A`) Assume only first step hydrolysis be significant.Given `,K_(a_(1)),K_(a_(2))& K_(a_(3))` For `H_(3)A` are `10^(-4),10^(-7) &10^(-9)` respectively.

Explanation

To calculate the pH of a 0.1 M solution of the salt of a tribasic acid \( H_3A \), we will consider only the first step of hydrolysis. The given dissociation constants are \( K_{a1} = 10^{-4} \), \( K_{a2} = 10^{-7} \), and \( K_{a3} = 10^{-9} \).

### Step-by-Step Solution:

1. **Identify the relevant equilibrium**:
The salt \( Na_3A \) will hydrolyze in water to produce \( OH^- \) ions:
\[
Na_3A + H_2O \rightleftharpoons Na^+ + H_2A^- + OH^-
...