When ethyl acetate was hydrolysed in presence of 0.1 N. HCl , the rate constant was found to be 5.40 × 10-5 s -1 But when 0.1 N H 2 SO 4 was used for the hydrolysis, the rate constant was found to be 6.20 × 10-5 s -1. From these values we can say that

Question

When ethyl acetate was hydrolysed in presence of 0.1 N. HCl , the rate constant was found to be 5.40 × 10-5 s -1 But when 0.1 N H 2 SO 4 was used for the hydrolysis, the rate constant was found to be 6.20 × 10-5 s -1. From these values we can say that (A) H 2 SO 4 is stronger than HCl (B) H 2 SO 4 is weaker than HCl (C) both the acids have equal strength (D) the data is insufficient to compare the strengths of HCl and H 2 SO 4

Tardigrade Admin · Accepted Answer

For equinormal solutions of the two acids, ( text Strength of Acid 1/ text Strength of Acid 2)=(k1/k2)

Q. When ethyl acetate was hydrolysed in presence of $0.1 N$ . $H Cl$ , the rate constant was found to be $5.40 \times 1 0^{- 5} s^{- 1}$ But when $0.1 N H_{2} S O_{4}$ was used for the hydrolysis, the rate constant was found to be $6.20 \times 1 0^{- 5} s^{- 1}$ . From these values we can say that

$H_{2} S O_{4}$ is stronger than $H Cl$

$H_{2} S O_{4}$ is weaker than $H Cl$

both the acids have equal strength

the data is insufficient to compare the strengths of $H Cl$ and $H_{2} S O_{4}$

For equinormal solutions of the two acids,

$\frac{Strength of Acid _{1}}{Strength of A c i d _{2}} = \frac{k _{1}}{k _{2}}$

Q. When ethyl acetate was hydrolysed in presence of 0.1N. HCl, the rate constant was found to be 5.40×10−5s−1 But when 0.1NH2​SO4​ was used for the hydrolysis, the rate constant was found to be 6.20×10−5s−1. From these values we can say that

H2​SO4​ is stronger than HCl

H2​SO4​ is weaker than HCl