A buffer solution containing `0.25mol//L` of `NH_(4)CI` and `0.05mol//L` of `NH_(4)OH` is in equilibrium with `A1^(+3)` and `Mg^(2+)` ions. Calculate `[A1^(3+)]` and `[Mg^(2+)]` in solution.
`K_(b)(NH_(4)OH) = 2.0 xx 10^(-5), K_(sp)[Mg(OH)_(2)] = 6.0 xx 10^(-12), 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) A1(OH)_(3) = 6 xx 10^(-32) .

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

Calculate pH of saturated solution Mg(OH)_(2),K_(sp) for Mg(OH)_(2) is 8.9 xx 10^(-12) .

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

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .

Should Mg(OH)_(2) precipitate from a solution that is 0.01 M MgCl_(2) if the solution is also made 0.10 M in NH_(3)[K_((sp)[Mg(OH)_(2)])=1.8 xx10^(-11) , K_(b(NH_(4)OH))= 1.8 xx 10^(-5)]

To a solution of 0.01M Mg^(2+) and 0.8M NH_(4)CI , and equal volume of NH_(3) is added which just gives precipitates. Calculate [NH_(3)] in solution. K_(sp) of Mg(OH)_(2) = 1.4 xx 10^(-11) and K_(b) of NH_(4)OH = 1.8 xx 10^(-5) .