Determine pH of 0.558M `H_2SO_3` solution given `K_(a1)` = 1.7x`10^(-2)` , K_(a2)` = `10^(-8)

The [H^(+)] of 0.10 MH_(2)S solution is (given K_(1)=1.0 xx 10^(-7) , K_(2)=1.0 xx 10^(-14))

Calculate the pH of 0.02 M H_2S (aq) given that K_(a_1)=1.3xx10^(-7), K_(a_2)=7.1xx10^(-15)

What is the pH of 0.01 M glycine solution? For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K