Calculate the degree of hydrolysis and `pH` of `0.2M` solution of `NH_(4)C1` Given `K_(b)` for `NH_(4)OH` is `1.8 xx 10^(-5)`.

Calculate the degree of hydrolysis of 0.04 M solution of NH_(4) CI" of " pH =5.28

Calculate the degree of hydrolysis and hydrolysis constant of 0.01 M solution of NH_(4)CI . Given K_(w) =1 xx 10^(-14) , K_(b) =1.75 xx 10^(-5)

Calculate [OH^(-)] in 0.20M solution of NH_(3) , if K_(b) for NH_(3) is 1.8xx10^(-5) .

Calculate degree of hydrolysis and pH of 0.25 NaCN solution at 25^@C . K_a=4.8xx10^(-10)

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 degree of hydrolysi and the pH of 0.02 M ammonium cyanide solution 298 K. K_b(NH_4OH)=1.77xx10^(-5) , K_a(HCN)=4.99xx10^(-10)

Calculate the hydrolysis constant and degree of hydrolysis of NH_(4) Cl" in " 0.1 M solution . K_(b) = 1.8 xx 10^(-5) . Calculate the concentration of H^(+) ions in the solution .

Calculate the pH of 0.10 M solution of Nh_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8xx10^(-5)