One litre of a buffer solution contains `0.1 M NH_(4)OH`. The `p^(kb)` of base is `5.pH` value of the solution is

1 lit of buffer solution contains 0.1 mole each of NH_(4)OH and NH_(4)Cl . What will be the P^(H) of the solution when 0.01 mole of HCl is added to it [ P^(Kb) of NH_(4)OH = 4.74 ]

One litre a butter solution containing 0.01 M NH_(4)Cl and 0.1 M NH_(4)OH having pk_(b) of 5 has Ph of

A buffer solution contains 0.3 mol dm-3 NH_4OH is 1.8 xx10^-5 .Calculate pOH of the solution.

The pH of a buffer solution of 0.1 M NH_(4)OH [ pK_(a)=4.0] and 0.1 M NH_(4)Cl is

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) .

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. b. How much NaOH should be added to 1L of the solution to change pH by 0.6.K_(b) =2xx10^(-5) .

A buffer solution contains 0.02 moles of NH_4OH and 0.03 moles of NH_4CI dissolved in 1 litre of the solution. Calculate the pH of the solution. Dissociation constant of NH_4OH "is" 1.8 xx 10^-5

A buffer solution has equal volumes of 0.2 M NH_(4)OH and 0.02 M NH_(4) CI The pk_(b) of the base is 5. The pH is

A buffer solution has equal volume of 0.20 M NH_(4)OH and 0.02 MNH_(4)Cl : The pK_(b) of the base is 5. The pH is