Calculate `[H^(o+)], [C_(3)H_(5)O_(3)^(Θ)]`, and `[PhO^(Θ)]` in a solution that is `0.03M (C_(2)H_(5)overset(O)overset(||)(C)-O-O-H)` and `0.1MPhOH? K_(a)` values for `C_(3)H_(5)O_(3)H` and `PhOH` are `1.48 xx 10^(-4)` and `1.05 xx 10^(-10)` respectively.

Explanation

To solve the problem, we need to find the concentrations of \( [H^+] \), \( [C_3H_5O_3^-] \), and \( [PhO^-] \) in a solution that contains \( 0.03 \, M \) of \( C_3H_5O_3H \) (which is a weak acid) and \( 0.1 \, M \) of phenol (\( PhOH \)). The \( K_a \) values for \( C_3H_5O_3H \) and \( PhOH \) are given as \( 1.48 \times 10^{-4} \) and \( 1.05 \times 10^{-10} \) respectively.

### Step 1: Calculate \( [H^+] \) from \( C_3H_5O_3H \)

Since \( C_3H_5O_3H \) is a weak acid, we can use the formula for the dissociation of a weak acid:
\[ K_a = \frac{[H^+][C_3H_5O_3^-]}{[C_3H_5O_3H]} \]
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