The rate equation for the acid-catalysed hydrolysis of methyl ethanoate is:
rate=k[H+][CH3COOCH3] \text{rate} = k [\text{H}^+] [\text{CH}_3\text{COOCH}_3] rate=k[H+][CH3COOCH3]The rate of reaction was measured for a mixture of methyl ethanoate and hydrochloric acid at pH=1.30\text{pH} = 1.30pH=1.30.
In a second mixture, the concentration of the hydrochloric acid was different but the concentration of methyl ethanoate was unchanged. The new rate of reaction was a fifth of the original rate.
What was the pH\text{pH}pH of the second mixture?
