Approximate pH of 0.01 M NaHA is calculated by :
`(K_(a1)=10^(-6)` and `K_(a2)=10^(-8)` are ionization constants of `H_(2)A)`

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

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)

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

Successive dissociation constants of H_(2)CO_(3) are K_(a_(1)) = 10^(-3) and K_(a_(2)) = 10^(-6) . An aqueous solution contains 0.1 MH_(2)CO_(3) and 0.1 M HCI at 25^(@)C The concentration of CO_(3)^(2-) at equilibrium in solution is: (approximately)

Calculate the pH when equal volume of 0.01 M HA (K_(a) = 10^(-6)) and 10^(-3)M HB (K_(a) = 10^(-5)) are mixed.

Calculate PH Of 0.01 M acetic acid . K_a = 1.8 xx 10^-5 at 298 K.

Calculate pH of a resultant solution of 0.1 M HA (K_(a)=10^(-6)) and 0.5 M HB (K_(a)=2xx10^(-6)) at 25^(@)C.

Calculate pH of a resultant solution of 0.1 M HA (K_(a)=10^(-6)) and 0.5 M HB (K_(a)=2xx10^(-6)) at 25^(@)C.

Calculate pH of a resultant solution of 0.1 M HA (K_(a)=10^(-6)) and 0.45 M HB (K_(a)=2xx10^(-6)) at 25^(@)C.

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. )