[" late the "pH" of "0.010MNaHCO_(3)" solution."],[4.5times10^(-7);K_(a2)=4.7times10^(-11)for" carbonic acid "]

Calculate the pH of 0.010M NaHCO_(3) solution. K_(1)=4.5xx10^(-7) , K_(2)= 4.7xx10^(-11) for carbonic acid.

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

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

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))

Find pH of 0.1 M NaHCO_(3) ?K1=5*10^-7, K2=5*10^-11 for carbonic acids.

[" pH of "0.5M" solution of sodium nitrite in water."(K_(a)" of "HNO_(2)-7times10^(-4))" (Assume "1],[-a-1)]

The PH of 10^(-2)MNH_(4)CN solution would be- (Given that K_(a) of HCN=5times10^(-10) and K_(b) of ( ) agNH_(3) ) =2times10^(-5) )