Find moles of `NH_(4)Cl` required to prevent `Mg(OH)_(2)` from precipitating in a litre of solution which contains 0.02 mole `NH_(3)` and 0.001 mole `Mg^(2+)` ions.
Given : `K_(b)(NH_(3))=10^(-5),` `K_(sp)[Mg(OH)_(2)]=10^(-11)`.

Calculate [overset(o+)NH_(4)] (derived from NH_(4)C1) needed to prevent Mg(OH)_(2) from precipitating is 1.0L of solution which contins 0.01mol NH_(3) and 0.001 mol Mg^(2+). K_(sp) Mg(OH)_(2) = 1.2 xx 10^(-11), K_(b) NH_(3) = 1.8 xx 10^(-5) .

How many millimoles of MgCI_(2) should be added to just precipitate Mg(OH) in 500 ml buffer solution containing 0.1 M NH_(4)OH and 0.1M(NH_(4))_(2)SO_(4) ? {Given : K_(b) (NH_(4)OH) = 10^(-5), K_(sp) [Mg(OH)_(2)] = 10^(-11)}

Which of the following concentration of NH_(4)^(+) will be sufficient to present the precipitation of Mg(OH)_(2) form a solution which is 0.01 M MgCl_(2) and 0.1 M NH_(3)(aq) . Given that K_(sp)Mg(OH)_(2)=2.5xx10^(-11) and K_(b) for NH_(3) = 2xx10^(-5) .

Which of the following concentration of NH_(4)^(+) will be sufficient to present the precipitation of Mg(OH)_(2) form a solution which is 0.01 M MgCl_(2) and 0.1 M NH_(3)(aq) . Given that K_(sp)Mg(OH)_(2)=2.5xx10^(-11) and K_(b) for NH_(3) = 2xx10^(-5) .

Calculate the pH of a buffer solution containing 0.2 mole of NH_4Cl and 0.1 mole of NH_4OH per litre. K_b for NH_4OH=1.85xx10^(-5) .

What is the maximum concentration of Mg^(+2) that can be introduced into a solution containing 0.1 M NH_3 and 0.01 M NH_4^(+ ) without causing precipitation of Mg (OH)_2 ? K_b of NH_3 = 10^(6) K_(sp) of Mg(OH)_2 =1.2 xx 10^(-12)