Concentration of `CN^(-) " in " 0.1` M HCN is (Given :`K_(a) = 4 xx 10^(-10)`)

The increasing order of Ag^(+) ion concentration in I. Saturated solution of AgCl II. Saturated solution of Agl III. 1MAg(NH_(3))_(2)^(+)" in "0.1 M NH_(3) IV. 1MAg(CN)_(2)^(-)" in "0.1 M KCN Given : K_(sp)" of "AgCl=1.0xx10^(-10) K_(sp)" of "Agl=1.0xx10^(-16) K_(d)" of "Ag(NH_(3))_(2)^(+)=1.0xx10^(-8) K_(d)" of "Ag(CN)_(2)^(-)=1.0xx10^(-21)

The increasing order of Ag^(+) ion concentration in I. Saturated solution of AgCl II. Saturated solution of Agl III. 1MAg(NH_(3))_(2)^(+)" in "0.1 M NH_(3) IV. 1MAg(CN)_(2)^(-)" in "0.1 M KCN Given : K_(sp)" of "AgCl=1.0xx10^(-10) K_(sp)" of "Agl=1.0xx10^(-16) K_(d)" of "Ag(NH_(3))_(2)^(+)=1.0xx10^(-8) K_(d)" of "Ag(CN)_(2)^(-)=1.0xx10^(-21)

Calculate the concentration of all species of significant concentrations presents in 0.1 M H_(3)PO_(4) solution. lf K_(1) = 7.5 xx 10^(-3), K_(2) = 6.2 xx 10^(-8), K_(3) = 3.6 xx 10^(-13)

What amount of HCl will be required to prepare one litre of a buffer solution of pH 10.4 using 0.01 mole of NaCN ? Given K_(ion)(HCN)=4.1xx10^(-10) .

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