The hydrolysis of ethyl acetate
`CH_(3)COOC_(2)H_(3)+H_(2)O hArr CH_(3) COOH + C_(2)H_(5)OH`
in aqueous solution is first order with respect to ethyl acetate. Upon varying the pH of the solution the first order rate constant varies as follows.
`pH" "3" "2" "1`
`k_(1)xx10^(-4)s^(-1)" "1.1" "11" "110`
what is the order of the reaction with respect of `H^(+)` and the value of the rate constant ?

Explanation

To solve the problem regarding the hydrolysis of ethyl acetate and determine the order of the reaction with respect to \( H^+ \) ions and the value of the rate constant, we can follow these steps:

### Step 1: Understand the Reaction
The hydrolysis reaction is given as:
\[ CH_3COOC_2H_5 + H_2O \rightleftharpoons CH_3COOH + C_2H_5OH \]
This reaction is first order with respect to ethyl acetate.

### Step 2: Analyze the Rate Constant Variation with pH
...