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

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)

Calculate the pH of 0.10 M solution of NH_4CI . The dissociation constant (K_b) "of" NH_3 "is" 1.8 xx 10^(-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).

Calcuate the degree of ionisation and pH of 0.05 M solution of a weak base having the ionization constant (K_(b)) is 1.77xx10^(-5). Also calculate the ionisation constant of the conjugate acid of this base.

Calculate the pH of 0.01 M Solution of CH_3 COOH . The dissociation constant of the acid is 1.8 xx 10 ^(-5)

The pH value of 0.20 M solution of CH_3NH_2 at 298 K is [Given that its ionisation constant K_b is 5.0xx10^-5 ]

Determine the hydrogen ion concentration in 1.0 M solution of HCN , if its dissociation constant is 4.0 xx 10^(-10) .

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?

The pH of a solution of NH_4Cl is 4.86 .Calculate the molar concentration fo the solution if K_b= 1.0 xx 10^(-5) and K_w = 1.0 xx 10 ^(-14)