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)` )
(A) 8.7
(B) 9.2
(C) 11.2
(D) 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).

Calculate the pH of 0.1 MNH_(3) solution. K_(b) = 1.8 ** 10^(-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?

What will be the pH and % alpha ( degree of hydrolysis ) respectively for the salt BA of 0.1M concentration ? Given : K_(a) for HA=10^(-6) and K_(b) for BOH=10^(-6) (a) 5,1% (b) 7, 10% (c) 9, 0.01% (d) 7, 0.01%

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) .

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 pH of a solution of ammonium acetate (Given : K_a= 1.78 xx 10 ^(-5) ,K_b= 1.8 xx 10 ^(-5) and K_w = 1.8 xx 10^(-14))