Let the solubilities of AgCl in H2 O, 0.01 M CaCl2; 0.01 M NaCl and 0.05 M AgNO3 be S1, S2, S3

step 1 Dear students in problem 143 of chapter 7 we've asked that let the solubilities of AGCL in H2O i

Let the solubilities of AgCl in H2 O, 0.01 M CaCl2; 0.01 M...

Let the solubilities of $\mathrm{AgCl}$ in $\mathrm{H}_{2} \mathrm{O}, 0.01 \mathrm{M} \mathrm{CaCl}_{2}$; $0.01 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M} \mathrm{AgNO}_{3}$ be $\mathrm{S}_{1}, \mathrm{~S}_{2}, \mathrm{~S}_{3}$ and $\mathrm{S}_{4}$ respectively. What is the correct relationship between these quantities? (1) $S_{1}>S_{2}>S_{3}>S_{4}$ (2) $S_{1}>S_{2}=S_{3}>S_{4}$ (3) $S_{1}>S_{3}>S_{2}>S_{4}$ (4) $S_{4}>S_{2}>S_{3}>S_{1}$

Let the solubilities of $\mathrm{AgCl}$ in $\mathrm{H}_{2} \mathrm{O}, 0.01 \mathrm{M} \mathrm{CaCl}_{2}$;
$0.01 \mathrm{M} \mathrm{NaCl}$ and $0.05 \mathrm{M} \mathrm{AgNO}_{3}$ be $\mathrm{S}_{1}, \mathrm{~S}_{2}, \mathrm{~S}_{3}$ and $\mathrm{S}_{4}$
respectively. What is the correct relationship between these quantities?
(1) $S_{1}>S_{2}>S_{3}>S_{4}$
(2) $S_{1}>S_{2}=S_{3}>S_{4}$
(3) $S_{1}>S_{3}>S_{2}>S_{4}$
(4) $S_{4}>S_{2}>S_{3}>S_{1}$

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Key Concepts

Solubility Equilibrium

This concept involves the balance between a sparingly soluble salt and its ions in solution, determined by its solubility product constant (Ksp). Understanding solubility equilibrium helps in calculating the concentration of ions in solution when the salt dissolves and explains how equilibrium is affected when additional ions are introduced into the system.

Common Ion Effect

The common ion effect describes the decrease in solubility of a salt when a solution already contains one of the ions present in that salt. In the context of sparingly soluble salts, adding a common ion shifts the dissolution equilibrium towards the undissolved salt, reducing its solubility. This concept is essential when comparing solubility under different conditions where additional sources of common ions are present.

Influence of Salt Composition on Ion Concentration

This concept examines how the composition and concentration of added salts contribute to the overall concentration of common ions in solution. For instance, salts that provide multiple equivalents of a common ion will have a different impact on solubility compared to those that furnish a single equivalent. Understanding this helps predict how the presence and concentration of different salts modify the solubility of a sparingly soluble compound.

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