`0.1 M H_(2)S` has `K_(1)=10^(-5) & K_(2)=1.5xx10^(-12)`. What will be the concentration of `S^(-2)` in the solution.

K_(1) and K_(2) for dissociation of H_(2)A are 4xx10^(-3) and 1xx10^(-5) . Calculate concentration of A^(2-) ion in 0.1M H_(2)A solution. Also report [H^(+)] and pH.

K_(1) and K_(2) for dissociation of H_(2)A are 4xx10^(-3) and 1xx10^(-5) . Calculate concentration of A^(2-) ion in 0.1M H_(2)A solution. Also report [H^(+)] and pH.

A solution contains 0.1M H_2S and 0.3M HCI. If K_a and K_(a2) for H_2 S are 1 xx 10^(-7) and 1.3 xx 10^(-13) respectively, calculate concentration of HS^- and S^- in the mixture.

(x)/(20)M concentration of H^(+) ion must be maintained in a saturate H_(2)S(0.1M) to precipitates CdS but not ZnZ, if [Cd^(2+)]=[Zn^(2+)]=0.1M initially. K_(sp)(CdS)=8xx10^(-27), K_(sp)(ZnS)=1xx10^(-21)K_(a)(H_(2)S)=1xx10^(-21)ZnS will not precipitate at concentration of H^(+) greater than (x)/(20)M . The value of x is .

If a solution is 0.1M with respect to H_(2)S and 0.5M with respect to HCI then the concetration of [S^(2-)] in the solution is x xx 10^(-22)M .Find the value of x. Given : {:(K_(a_(1)) = 10^(-7)),(K_(a_(2)) = 10^(-14)):}]H_(2)S

A solution contains 0.10 M H_2S and 0.3 HCl Calculate the concentration of S^(2-) and HS^(-) ions in the solution . For H_2S , K_(a_1) = 1 xx 10^(-7) and K_(a_2) = 1.3 xx 10^(-13)

A solution contains 0.1MH_(2) and 0.3MHCl. Calculate the concentration of S^(2) and HS- ions in the solution. For H_(2)S, K_(a_(1))=1.05xx10^(-7) and K_(a_(2))=1.3xx10^(-14) .

A solution containing both Zn^(2+) and Mn^(2+) ions at a concentration of 0.01M is saturated with H_(2)S . What is pH at which MnS will form a ppt ? Under these conditions what will be the concentration of Zn^(2+) ions remaining in the solution ? Given K_(sp) of ZnS is 10^(-22) and K_(sp) of MnS is 5.6 xx 10^(-16), K_(1) xx K_(2) of H_(2)S = 1.10 xx 10^(-21) .