Calculate `[H^(o+)]` in a soluton that is `0.1M HCOOH` and `0.1 M HOCN. K_(a)(HCOOH) = 1.8 xx 10^(-4), K_(a) (HoCN) = 3.3 xx 10^(-4)`.

Explanation

To calculate the concentration of hydrogen ions \([H^+]\) in a solution that is \(0.1 \, M\) in both formic acid (HCOOH) and cyanic acid (HOCN), we will follow these steps:

### Step 1: Write the dissociation equations for both acids
1. **For formic acid (HCOOH)**:
\[ \text{HCOOH} \rightleftharpoons \text{H}^+ + \text{HCOO}^- \]
The dissociation constant \(K_a\) for HCOOH is given as \(1.8 \times 10^{-4}\).
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