Calculate the concentration of all species of significant concentrations presents in `0.1 M H_(3)PO_(4)` solution. lf `K_(1) = 7.5 xx 10^(-3), K_(2) = 6.2 xx 10^(-8), K_(3) = 3.6 xx 10^(-13)`

Explanation

To calculate the concentration of all species present in a 0.1 M solution of \( H_3PO_4 \), we will follow the steps of dissociation of the acid and use the provided dissociation constants \( K_1, K_2, \) and \( K_3 \).

### Step 1: Write the dissociation reactions and equilibrium expressions

1. **First dissociation:**
\[ H_3PO_4 \rightleftharpoons H^+ + H_2PO_4^- \]
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