What is the pH of `10^(-3)` M ammonia cyanide solution, if `K_(HCN)=7.2 xx 10^(-11)` and `K_(NH_(3))=1.8 xx 10^(-5)mol L^(-1)` ?

What is the pH of 0.01 M glycine solution? For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K

What is the pH of 0.01 M glycine solution? [For glycine, K_(a_(1))=4.5xx10^(-3) and K_(a_(2))=1.7xx10^(-10) at 298 K ]

Calculate the solubility og AgCN in a buffer solution of pH 3.00 K_(sp(AgCN)) = 1.2 xx10^(-18) and K_(a(HCN)) = 4.8 xx 10^(10) M^(2) .

The P^(H) of an aqueous solution of NH_4 CN( K_a of HCN is 9.2 xx 10^(-10) & K_b of NH_4 OH is 1.8 xx 10^(-5))

Calculate the drgee of hydrolysis and pH of 0.02M ammonium cyanide (NH_(4)CN) at 298K . (K_(a) of HCN = 4.99 xx 10^(-9), K_(b) for NH_(4)OH = 1.77 xx 10^(-5))

Calculate the dergee of hydrolysis and pH of 0.02M ammonium cyanide (NH_(4)CN) at 298K . (K_(a) of HCN = 4.99 xx 10^(-9), K_(b) for NH_(4)OH = 1.77 xx 10^(-5))