The density of `NH_(4)OH` solution is `0.6g//mL`. It contains `34%` by weight of `NH_(4)OH`. Calculate the normality of the solution:

The density of NH_4OH solution is found to be 0.6 g/ml. It contains 34% by weight of NH_4OH . Calculate the normality of the solution.

Equivalent weight of NH_(4)OH is

If density of NH_(4)OH solution is 1g/ml and it is 35% w/v . Calculate the normality of the solution

Ammonia gas is passed into water, yielding a solution of density 0.93 g//cm^(3) and containing 18.6% NH_(3) by weight. The mass of NH3 per cc of the solution is :

Ammonia gas is passed into water, yielding a solution of density 0.93 g//cm^(3) and containing 18.6% NH_(3) by weight. The mass of NH3 per cc of the solution is :

Ammonia gas is passed into water, yielding a solution of density 0.93 g//cm^(3) and containing 18.6% NH_(3) by weight. The mass of NH3 per cc of the solution 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: Molar conductivity of 0.1 M NH_(4)OH solution is less than that of 0.001 M NH_(4)OH solution. R: Dilution increases the degree of ionisation of NH_(4)OH