What concentration of `OH^(-)` ions will reduce `NH_(4)^(+)` ion to `2xx10^(-5)M` in `0.4M` solution of `NH_(4)OH ? K(b)(NH_(4)OH)=1.8xx10^(-5)`

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

The pH of a 0.1 M solution of NH_(4)OH (having K_(b)=1.0xx10^(-5)) is equal to

Calculate the concentration of OH^_ ions of 0.01 M NH_4OH : K_b = 1.58 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 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) .

0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH^(-) ion concentration of this solution ? (K_(b) (NH_(4) OH) = 1.8 xx 10^(-5)

0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH^(-) ion concentration of this solution ? (K_(b) (NH_(4) OH) = 1.8 xx 10^(-5)

Freshly precipiteated Al and Mg hydroxides are stirred vigorously in a buffer solution containing 0.25M of NH_(4)CI and 0.05M of NH_(4)OH . Calculate [Al^(3+)] and [Mg^(2+)] in solution. K_(b) for NH_(4)OH=1.8xx10^(-5) K_(SP) of Al(OH)_(3)=6xx10^(-32) and K_(SP) of Mg(OH)_(2)=8.9xx10^(-12) .

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )