Find the pH of `" 0.1 M NaHCO_(3)"`.
Use data `(K_(1)=4xx10^(-7),K_(2)=4xx10^(-11)` for `H_(2)CO_(3), log 4=0.6) :`

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

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

Find the DeltapH( initial pH - final pH) when 100 ml 0.01M HCl is added in a solution containing 0.1m moles of NaHCO_(3) solution of negligible volume (k_(a_(1))=10^(-7),k_(a_(2))=10^(-11) for H_(2)CO_(3)) :

50 ml, 0.1M NaHCO_(3) aqueous solution is mixed with 50 ml, 0.8 M Na_(2)CO_(3) aqueous solution at 25^(@)C . The pH of resulting solution exiists between colour transition range of an indicator which is: (K_(a_(1))=4xx10^(-7), K_(a_(2)) =2xx10^(-11) "for" H_(2)CO_(3))

50 ml, 0.1M NaHCO_(3) aqueous solution is mixed with 50 ml, 0.8 M Na_(2)CO_(3) aqueous solution at 25^(@)C . The pH of resulting solution exiists between colour transition range of an indicator which is: (K_(a_(1))=4xx10^(-7), K_(a_(2)) =2xx10^(-11) "for" H_(2)CO_(3))

The pH of 2.5xx10^(-1) M HCN solution (K_(a)=4xx10^(-10)) is :

The pH of 0.1 M NaHCO_(3) is (Given K_(a1) and K_(a2) for H_(2)CO_(3) are 6.38 and 10.26 respectively. )

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