For the following two acid-base reactions,whi | vedclass

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(A) An acid-base reaction always proceeds in the direction of the formation of the weaker acid and weaker base.For reaction $(I)$:Acid on left is $CH_

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$I$ is favoured to the right,$II$ is favoured to the left

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(A) An acid-base reaction always proceeds in the direction of the formation of the weaker acid and weaker base.For reaction $(I)$:Acid on left is $CH_3NH_2$ $(pK_a = 35)$ and acid on right is $CH_3CH_3$ $(pK_a = 50)$.Since $50 > 35$,$CH_3CH_3$ is a weaker acid than $CH_3NH_2$. Thus,the equilibrium is favoured to the right.For reaction $(II)$:Acid on left is $H_2O$ $(pK_a = 15.7)$ and acid on right is $HF$ $(pK_a = 3.2)$.Since $15.7 > 3.2$,$H_2O$ is a weaker acid than $HF$. Thus,the equilibrium is favoured to the left.

For the following two acid-base reactions,which statement is True?
$(I) CH_3CH_2^- + CH_3NH_2$ $(pK_a = 35)$ $\rightleftharpoons CH_3CH_3$ $(pK_a = 50)$ $+ CH_3NH^-$
$(II) F^- + H_2O$ $(pK_a = 15.7)$ $\rightleftharpoons HF$ $(pK_a = 3.2)$ $+ HO^-$

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For the following two acid-base reactions,which statement is True?$(I) CH_3CH_2^- + CH_3NH_2$ $(pK_a = 35)$ $\rightleftharpoons CH_3CH_3$ $(pK_a = 50)$ $+ CH_3NH^-$$(II) F^- + H_2O$ $(pK_a = 15.7)$ $\rightleftharpoons HF$ $(pK_a = 3.2)$ $+ HO^-$