How many times solubility of CaF2 is decreased in 4 ×10^-3 M-KF(aq) solution as compared to pure

step 1 Hello students for this question we are given the solubility to be equal to 17 into 10 to the pe

How many times solubility of CaF2 is decreased in 4 ×10^-3...

How many times solubility of $\mathrm{CaF}_{2}$ is decreased in $4 \times 10^{-3} \mathrm{M}-\mathrm{KF}(\mathrm{aq})$ solution as compared to pure water at $25^{\circ} \mathrm{C}$. Given:
$K_{\text {sp }}\left(\mathrm{CaF}_{2}\right)=3.2 \times 10^{-11}$
(a) 50
(b) 100
(c) 500
(d) 1000

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Key Concepts

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is a specific type of equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It represents the product of the concentrations of the ions each raised to the power of its stoichiometric coefficient when the solid is in dynamic equilibrium with its ions in solution. Ksp is a crucial parameter in determining how readily a salt dissolves in water and is widely used in solubility calculations and precipitation predictions.

Common Ion Effect

The common ion effect is the phenomenon where the solubility of a sparingly soluble salt is reduced when a solution already contains one of the ions present in the salt. The presence of the common ion shifts the equilibrium position according to Le Chatelier’s principle, favoring precipitation of the salt and resulting in lower overall solubility. This concept is essential for understanding how the addition of electrolytes influences solubility in aqueous solutions.

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