Silver ions are slowly added in a solution with [Br^-]=[Cl^-]=[CO3^2-]=[AsO4^3-] =0.1 M. Which c

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Silver ions are slowly added in a solution with...

Silver ions are slowly added in a solution with $\left[\mathrm{Br}^{-}\right]=\left[\mathrm{Cl}^{-}\right]=\left[\mathrm{CO}_{3}^{2-}\right]=\left[\mathrm{AsO}_{4}^{3-}\right]$ $=0.1 \mathrm{M}$. Which compound will precipitate first? (a) $\operatorname{AgBr}\left(K_{\mathrm{sp}}=5 \times 10^{-13}\right)$ (b) $\mathrm{AgCl}\left(K_{\mathrm{sp}}=1.8 \times 10^{-10}\right)$ (c) $\mathrm{Ag}_{2} \mathrm{CO}_{3}\left(K_{\mathrm{sp}}=8.1 \times 10^{-12}\right)$ (d) $\mathrm{Ag}_{3} \mathrm{PO}_{4}\left(K_{\mathrm{sp}}=1 \times 10^{-22}\right)$

Silver ions are slowly added in a solution with $\left[\mathrm{Br}^{-}\right]=\left[\mathrm{Cl}^{-}\right]=\left[\mathrm{CO}_{3}^{2-}\right]=\left[\mathrm{AsO}_{4}^{3-}\right]$
$=0.1 \mathrm{M}$. Which compound will precipitate first?
(a) $\operatorname{AgBr}\left(K_{\mathrm{sp}}=5 \times 10^{-13}\right)$
(b) $\mathrm{AgCl}\left(K_{\mathrm{sp}}=1.8 \times 10^{-10}\right)$
(c) $\mathrm{Ag}_{2} \mathrm{CO}_{3}\left(K_{\mathrm{sp}}=8.1 \times 10^{-12}\right)$
(d) $\mathrm{Ag}_{3} \mathrm{PO}_{4}\left(K_{\mathrm{sp}}=1 \times 10^{-22}\right)$

Key Concepts

Reaction Stoichiometry in Precipitation

The stoichiometry of the dissolution reaction determines how the concentration of each ion contributes to the overall ionic product. For salts that dissociate into more than one cation or anion, the exponent in the Ksp expression reflects that stoichiometry, which in turn affects the threshold concentration of a metal ion required to reach the point of precipitation.

Common Ion Effect

The common ion effect describes the change in solubility of a salt when a common ion is added to the solution. In a mixture containing several potential precipitating anions at the same concentration, the presence of the common ion influences the concentration of the other ion needed for precipitation, essentially raising the threshold concentration for precipitation of the salt sharing that ion.

Precipitation Reaction

A precipitation reaction occurs when the product of the concentrations of the ions in solution exceeds the solubility product (Ksp) for an insoluble compound, resulting in the formation of a solid. In systems with multiple potential precipitates, the one with the lowest ion concentration threshold (calculated by setting the ionic product equal to its Ksp) will begin to form first.

Solubility Product (Ksp)

The solubility product constant, Ksp, is an equilibrium constant that represents the product of the ionic concentrations of a sparingly soluble salt at saturation, each raised to the power of their coefficients in the balanced dissolution equation. It is used to predict whether a precipitate will form when two ionic solutions are mixed, by comparing the ionic product to the Ksp value.

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