The solubility product of PbI2 is 7.2 ×10^-9. The maximum mass of NaI which may be added in 500

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The solubility product of PbI2 is 7.2 ×10^-9. The maximum...

The solubility product of $\mathrm{PbI}_{2}$ is $7.2 \times 10^{-9}$. The maximum mass of NaI which may be added in $500 \mathrm{ml}$ of $0.005 \mathrm{M}-\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$ solution without any precipitation of $\mathrm{PbI}_{2}$ is $(\mathrm{I}=127)$ (a) $0.09 \mathrm{~g}$ (b) $1.2 \times 10^{-3} \mathrm{~g}$ (c) $6 \times 10^{-4} \mathrm{~g}$ (d) $1.08 \times 10^{-5} \mathrm{~g}$

The solubility product of $\mathrm{PbI}_{2}$ is $7.2 \times 10^{-9}$. The maximum mass of NaI which may be added in $500 \mathrm{ml}$ of $0.005 \mathrm{M}-\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$
solution without any precipitation of $\mathrm{PbI}_{2}$ is $(\mathrm{I}=127)$
(a) $0.09 \mathrm{~g}$
(b) $1.2 \times 10^{-3} \mathrm{~g}$
(c) $6 \times 10^{-4} \mathrm{~g}$
(d) $1.08 \times 10^{-5} \mathrm{~g}$

Key Concepts

Stoichiometric and Molarity Calculations

Stoichiometry and molarity calculations are used to convert between the amounts (in moles or mass) of reactants and products within a chemical reaction. In the context of precipitation and solubility, these calculations allow one to determine the amount of a reagent that can be added before exceeding the solubility limit, taking into account the volume of the solution and the molar relationships between the ions involved.

Precipitation Equilibrium

Precipitation equilibrium involves the balance between the dissolved ions and the solid precipitate. When the ionic product of a sparingly soluble salt exceeds its Ksp, excess ions combine to form a precipitate. Calculating the point at which the ionic product equals the Ksp helps determine the maximum concentration of ions that can be present in solution without causing precipitation.

Solubility Product (Ksp)

The solubility product constant (Ksp) is a special type of equilibrium constant that applies to the dissolution of a sparingly soluble salt. It represents the maximum product of the ion concentrations that can exist in solution before the salt begins to precipitate. Understanding Ksp is crucial for calculating whether a precipitate will form when different ionic species are present in solution.

Common Ion Effect

The common ion effect refers to the shift in equilibrium that occurs when an ion common to the solubility equilibrium is added to the solution. Adding an ion that is already a part of the dissolved salt’s equilibrium will typically reduce the solubility of that salt by driving the reaction toward the formation of the undissolved solid, thus influencing the concentration of available ions.

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