The rate law for the reaction ,
`CH_(3)COC_(2)H_(5)+H_(2)O overset([H^(+)]) toCH_(3)COOH +C_(2)H_(5)OH`
is `(dx)/(dt) =k [CH_(3)COOC_(2)H_(5)][H_(2)O]^(o)`
What will be the effect for the reaction ,
(ii) the concentration of `H^(+)` is tripled?

Explanation

To solve the problem regarding the effect of tripling the concentration of \( H^+ \) on the rate of the reaction:

1. **Identify the Rate Law**: The given rate law for the reaction is:
\[ \frac{dx}{dt} = k [CH_3COOC_2H_5][H_2O]^0 \]
Here, \( k \) is the rate constant, \( [CH_3COOC_2H_5] \) is the concentration of the ester, and \( [H_2O] \) is the concentration of water.

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