The PH of 10^(-2)MNH_(4)CN solution would be- (Given that K_(a) of HCN=5times10^(-10) and K_(b) of ( ) agNH_(3) ) =2times10^(-5) )

Calculate pH and degree of hydrolysis fo 10^(-2)MNH_(4)CN solution. Given that K_(a) of HCN=5xx10^(-10) and K_(b) of (aq. NH_(3))=2xx10^(-5) at 25^(@)C .

The pH of 0.02MNH_(4)Cl solution will be : [Given K_(b) (NH_(4)OH) = 10^(-5) and log 2 = 0.301 ]

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).

The Hydrolysis constant of MX is (Given, K_(b) of MOH is 2 xx 10^(-6) and K_(a) of HX is 5 xx 10^(-7) )

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) .

The [H^(+)] of 0.10 MH_(2)S solution is (given K_(1)=1.0 xx 10^(-7) , K_(2)=1.0 xx 10^(-14))

If K_(a) of HCN =4xx10^(-10) , then the pH of 2.4 xx 10^(-1) molar HCN(aq) is

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))