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 hydrolysis constant. Degree of hydrolysis and pH of 0.5 M solution of NH_4Cl. ( Given : K_a = 1.78 xx 10 ^(-5) ,K_b= 1.8 xx 10 ^(-5) and K_w = 1.8 xx 10 ^(-14) )

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 the hydrolysis constant. Degree of hydrolysis and pH of a 0.1 M NH_4Cl solution at 25 ^(@) C Given : K_b " for " NH_4OH= 1.8 xx 10^(-5)

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

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