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)`

What is the OH^(-) concentration of a 0.08 M solution of [K_(a)(CH_(3)COOH)=1.8 xx 10^(-5)]

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

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

Freshly prepared aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing 0.25M of ammonium chloride and 0.05M of ammonium hydroxide. Calculate the concentration of aluminium and magesium ions in solution (K_(b) NH_(4)OH = 1.8 xx 10^(-5), K_(sp) Mg(OH)_(2) = 6 xx 10^(-10), K_(sp) A1(OH)_(3) = 6 xx 10^(-32) .

Freshly prepared aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing 0.25M of ammonium chloride and 0.05M of ammonium hydroxide. Calculate the concentration of aluminium and magesium ions in solution (K_(b) NH_(4)OH = 1.8 xx 10^(-5), K_(sp) Mg(OH)_(2) = 6 xx 10^(-10), K_(sp) Al(OH)_(3) = 6 xx 10^(-32) .

The H^(+) ion concentration of a solution is 4xx10^(-5) M. Then the OH^(-) ion concentration of the same solution is

The H ion concentration of a solution is 4.75xx10^(-5) M. Then the OH ion concentration of the same solution is

The H^(+) ion concentration of a solution is 4 x 10^(-5) M. Then the OH^(-1) ion concentration of the same solution is