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Factors Affecting Alpha

Give reason I...

Question

Give reason In solution of $H_{2} S O_{4}$ in water, the seconds dissociation constant $K_{a 2}$ , is less than the first dissociation constant $K_{a 2}$ .

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Solution

${H_{2} S O_{4}}_{(a q)} + {H_{2} O}_{(l)} ⟶ {H_{3} O}^{+}_{(a q)} + {H S O_{4}}^{-}_{(a q)}; {K_{a}}_{1}$
${H S O_{4}}^{-}_{(a q)} + {H_{2} O}_{(l)} ⇌ {H_{3} O}^{+}_{(a q)} + {S O_{4}}^{2 -}_{(a q)}; {K_{a}}_{2}$
Acids have tendencies to lose the first proton easily but tends not to loose second proton in solution very easily.
Sulphuric acid, $(H_{2} S O_{4})$ loses one proton to form negatively charged ${H S O_{4}}^{-}$ ion which is a weaker acid as compared to sulphuric acid and therefore the second dissociation constant is less than the first dissociation constant.

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