The ratio of acid strength of `HOCN` and `HCN` is about
Given `K_(a)` of `HOCN=1.2xx10^(-4) and K_(a)" of "HCN "=4.2 xx10^(-10)`

Calculate the solubility of AgCN in a buffer solution of pH = 3 , Given K_(sp) of AgCN = 1.2 xx 10^(-16) and K_(a) for HCN = 4.8 xx 10^(-10) .

Calculate the ratio of degree of dissociation of acetic acid and hydrocyanic acid (HCN) in 1 M their respective solution of acids. ["Given "K_(a) (CH_(3)COOH)=1.8 xx 10^(-5) , K_(a(HCN))=6.2 xx 10^(-10)]

Calculate the pH of 0.01 M solution of NH_(4)CN. The dissociation constants K_(a) for HCN=6.2xx10^(-10)and K_(b) for NH_(3)=1.6xx10^(-5).

Calculate the pH of 0.01 M solution of NH_(4)CN. The dissociation constants K_(a) for HCN=6.2xx10^(-10)and K_(b) for NH_(3)=1.6xx10^(-5).

Calculate the pH of 0.01 M solution of NH_(4)CN. The dissociation constants K_(a) for HCN=6.2xx10^(-10)and K_(b) for NH_(3)=1.6xx10^(-5).

Calculate the solubility of AgCN in a buffer solution of pH 3.0 . Assume that no cyano complex is formed K_(sp) AgCN = 2.2 xx 10^(-16), K_(a) HCN = 6.2 xx 10^(-10) .

Calculate the solubility of AgCN in a buffer solution of pH 3.0 . Assume that no cyano complex is formed K_(sp) AgCN = 2.2 xx 10^(-16), K_(a) HCN = 6.2 xx 10^(-10) .

Equal volumes of 0.02M AgNO_(3) and 0.01M HCN are mixed. Calculate [Ag^(o+)] in solution after attaining equilibrium. K_(a) HCN = 6.2 xx 10^(-10) and K_(sp) of AgCN = 2.2 xx 10^(-16) .

Equal volumes of 0.02M AgNO_(3) and 0.01M HCN are mixed. Calculate [Ag^(o+)] in solution after attaining equilibrium. K_(a) HCN = 6.2 xx 10^(-10) and K_(sp) of AgCN = 2.2 xx 10^(-16) .

Calculate percentage hydrolysis in 0.003 M aqueous solution K_(a) for HOCN = 3.35 xx 10^(-4) and K_(w) = 10^(-14)