Why is Ka1=Ka2 for sulphuric acid in water

Q.

Why is for H₂SO₄ in water?

Q. Why is $K{a}_2<<K{a}_1$ for $H_{2}S{O}_4$ in water?

Q. Why is $K_{a2}$ $\ll$ $K_{a1}$ for $H_{2}S{O}_4$

Q. For a polybasic acid, the dissociation constants have different value for each steps, e.g.,
$H_{3}A\rightleftharpoons H^{+}+H_2{A}^{-};K=K_{a_1}$
$H_2{A}^{-}\rightleftharpoons H^{+}+H{A}^{2-};K=K_{a_2}$
$H{A}^{2-}\rightleftharpoons H^{+}+A^{3-};K=K_{a_3}$
What is the observed trend of dissociation constants in succesive stage?

Q. Sulphurous acid $\left(H_{2}S{O}_3\right)$ has $K_{a1}=1.7\times {10}^{-2}$ and $Ka2=6.4\times {10}^{-8}$. The pH of $0.588M{H}_{2}S{O}_3$ is ______ (Round off to the Nearest Integer).