In the acid hydrolyiss reaction `A + H_(2)O + H^(o+) rarr` Product, where `[H^(o+)] = 0.1 mol dm^(-3)` and `H_(2)O` is present in large excess, the apparent rate constant is `1.5 xx 10^(-5) s^(-1)`. Calculate the true rate constant.

Explanation

To solve the problem, we need to calculate the true rate constant (k) for the acid hydrolysis reaction given the apparent rate constant (k_apparent) and the concentrations of the reactants involved. Here are the steps to find the true rate constant:

### Step 1: Understand the Reaction
The reaction is given as:
\[ A + H_2O + H^+ \rightarrow \text{Product} \]
We know that the concentration of \( H^+ \) is given as \( [H^+] = 0.1 \, \text{mol dm}^{-3} \) and that water (\( H_2O \)) is in large excess.

### Step 2: Write the Rate Equation
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