Calculate the pH of `0.1 M NH_4 OH` if
`K_b =1.75 xx10^(-5)`.

Calculate the concentration of OH^_ ions of 0.01 M NH_4OH : K_b = 1.58 xx 10^(-5)

The pH of 0.10 M NH_(3) solution (K_(b)=1.8xx10^(-5)) is :

Calculate: (a) the hydrolysis constant (b) degree of hydrolysis, and (c) the pH of 0.01 M NH_4Cl at 25^@C . K_b(NH_4OH)=1.81xx10^(-5)

The pH of 10^(−3) M NH_4OH ( K_b =10^(−5) ) is:

Calculate the pH of 0.01 M NH_4Cl solution at 25^@C . K_b for NH_4OH=1.81xx10^(-5)

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. K_(b) =2xx10^(-5) .