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Question

The initial rate of hydrolysis methyl acetate (1 M) by a weak acid (HA, 1M) is 1/100th of that of a strong acid (HX, 1M), at 25oC. The Kaof HA is:

A
1 x 104
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B
1 x 105
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C
1 x 106
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D
1 x 103
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Solution

The correct option is A 1 x 104
The rate of the hydrolysis of methyl acetate is directly proportional to the hydrogen ion concentration.
In case of weak acid, the equilibrium constant is given by the expression Ka=[H+][A][HA]=[H+]2[HA]
Hence, [H+]=Ka[HA]

Hence, the expression for the ratio of the rate of the hydrolysis of methyl acetate in presence of weak acid and strong acid becomes rweakacidrstrongacid=Ka[HA][HA]=1100

Substitute [HA]=1M

Hence, Ka×11=1100
Ka=1×104

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