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 NH_4Cl solution at 25^@C . K_b for NH_4OH=1.81xx10^(-5)

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) )

if equal volume of O.1 M NH_4OH and 0.1 M HCl are mixed, then the pH of resulting mixture will be [Given pK_b (NH_4 OH)= 4.75, log 5=0.7)]

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 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 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)

The pH of 0.2 M aqueous solution of NH_4Cl will be (pK_b of NH_4OH = 4.74, log 2 = 0.3)

Calculate the number of moles of NH_(4)Cl that should be added to one litre of "1.0 M "NH_(4)OH to prepare buffer solution with pH=9[K_(b)=2xx10^(-5)," take log"2=0.3]