Solubility products of Mg(OH)2 , Cd(OH)2, Al(OH)3 and Zn(OH)2 are 4 ×10^-11, 8 ×10^

step 1 Dear students, in problem 18 of chapter 5th we have asked that the solubility product of ALOH 3

Solubility products of Mg(OH)2 , Cd(OH)2,...

$\begin{array}{llll}\text { Solubility } & \text { products of } & \mathrm{Mg}(\mathrm{OH})_{2} \text { , }\end{array}$ $\mathrm{Cd}(\mathrm{OH})_{2}, \mathrm{Al}(\mathrm{OH})_{3}$ and $\mathrm{Zn}(\mathrm{OH})_{2}$ are $4 \times 10^{-11}, 8 \times 10^{-6}, 8.5 \times 10^{-23}$ and $1.8 \times 10^{-14}$, respectively. The cation that will precipitate first as hydroxide, on adding limited quantity of $\mathrm{NH}_{4} \mathrm{OH}$ in a solution containing equimolar amount of metal cations, is (a) $\mathrm{Al}^{3+}$ (b) $\mathrm{Zn}^{2+}$ (c) $\mathrm{Mg}^{2+}$ (d) $\mathrm{Cd}^{2+}$

$\begin{array}{llll}\text { Solubility } & \text { products of } & \mathrm{Mg}(\mathrm{OH})_{2} \text { , }\end{array}$
$\mathrm{Cd}(\mathrm{OH})_{2}, \mathrm{Al}(\mathrm{OH})_{3}$ and $\mathrm{Zn}(\mathrm{OH})_{2}$ are
$4 \times 10^{-11}, 8 \times 10^{-6}, 8.5 \times 10^{-23}$ and
$1.8 \times 10^{-14}$, respectively. The cation that will precipitate first as hydroxide, on adding limited quantity of $\mathrm{NH}_{4} \mathrm{OH}$ in a solution containing equimolar amount of metal cations, is
(a) $\mathrm{Al}^{3+}$
(b) $\mathrm{Zn}^{2+}$
(c) $\mathrm{Mg}^{2+}$
(d) $\mathrm{Cd}^{2+}$

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Key Concepts

Selective Precipitation

Selective precipitation is a technique used to separate ions in a mixture by carefully controlling the conditions such that only one ionic species precipitates out at a specific point. This is achieved by gradually adding a precipitating agent and monitoring the ionic product relative to the Ksp values of the different compounds, ensuring that the ion with the lowest solubility threshold precipitates first.

Solubility Product (Ksp)

The solubility product is a constant that represents the maximum product of the ion concentrations for a sparingly soluble compound that can exist in equilibrium with its solid form. It is crucial for predicting when a precipitate will form in a solution, as a compound will begin to precipitate when the ionic product exceeds its Ksp value.

Precipitation Reaction

A precipitation reaction occurs when two soluble substances in solution react to form an insoluble compound, known as a precipitate. The formation of the precipitate is governed by the solubility product, and the reaction proceeds based on the relative concentrations of the ions involved.

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