The pH of `10^(-2)M` `NH_(4)CN` solution would be- (Given that `K_(a)` of HCN = `5times10^(-10)` and `K_(b)` of (`AgNH_(3))=2times10^(-5)` )
(1) 8.7
(2) 9.2
(3) 11.2
(4) 9.9

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

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).

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).

At what pH will a 1.0 xx 10^(-3)M solution of an indicator with K_(b) = 1.0 xx 10^(-10) changes colour?

Calculate the pH of 0.10 M solution of NH_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8 X 10^(-5)

The pH of a 0.1M solution of NH_(4)OH (having dissociation constant K_(b) = 1.0 xx 10^(-5)) is equal to

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

A solution is saturated with respect to SrCO_(3) and SrF_(2) . The [CO_(3)^(2-)] was found to be 1.2 xx 10^(-3)M . The concnetration of F^(Theta) in the solution would be Given K_(sp) of SrCO_(3) = 7.0 xx10^(-10)M^(2) , K_(sp) "of" SrF_(2) = 7.9 xx 10^(-10) M^(3) ,

Calculate the solubility of CaF_(2) in a solution buffered at pH = 3.0. K_(a) for HF = 6.3 xx 10^(-4) and K_(sp) of CaF_(2) = 3.45 xx 10^(-11) .