Silver chromate, Ag₂CrO₄ (Ksp=9.0×10−12), and silver chloride, AgCl (Ksp=1.8×10−10), are both slightly soluble salts of silver. Separate 100 mL samples of distilled water at 25 °C are placed in three beakers. To each beaker, 0.0100 mol of solid Ag₂CrO₄ is added and allowed to reach equilibrium. After equilibrium is established, the following reagents are added:
• Beaker 1: 5.00 mL of 1.00 M K₂CrO₄
• Beaker 2: 5.00 mL of 1.00 M NaCl
• Beaker 3: no additional reagent (control)
Assume volume changes are negligible.
(a) For each beaker, write the net ionic equation for any precipitation or dissolution process that may occur after the reagent is added (if any).
(b) Without performing extensive calculations, rank the three beakers in order of decreasing equilibrium concentration of Ag⁺ after the additions (highest [Ag⁺] to lowest [Ag⁺]).
(c) Provide a detailed justification for the ranking in part (b), explicitly addressing the relative impact of the two different common ions on the solubility of Ag₂CrO₄.
(d) In Beaker 2, some solid AgCl may also form. Describe qualitatively how the simultaneous presence of AgCl and Ag₂CrO₄ solids at equilibrium influences the final Ag⁺ concentration compared with a system in which only one silver salt is present.