Question

A precipitate of calcium oxalate will not dissolve in:
A. $HCl$
B. $HN{O_3}$
C. Aqua regia
D. $C{H_3}COOH$

Answer 1

Hint: We are aware that a substance's solubility in a particular solvent depends on the interactions between the solute and other solutes as well as the solvent and other solvents. The solubility also increases as the temperature rises. The amount of energy needed to disassemble an ionic lattice into its individual ions is known as lattice energy.

Complete Step by Step Solution:
When a weak electrolyte solution is combined with a strong electrolyte solution, a common ion effect is produced that produces an ion similar to the one produced by the weak electrolyte solution.

Oxalic acid dissociation is suppressed when strong acids, such as hydrochloric acid, nitric acid, and aqua regia, are added to a solution containing calcium oxalate because these acids give hydrogen ions (common ion effect). Consequently, the amount of oxalate ions is reduced.

Because the result of the ion concentrations in calcium oxalate will be less than the calcium oxalate's solubility result, the calcium oxalate precipitate will dissolve in it. Since acetic acid is a weak acid, the common ion effect is not seen when it is added. As a result, the calcium oxalate precipitate will not dissolve.
So, the correct option is D.

Note: Since it is a stronger acid than acetic acid, the oxalic salts have not been broken down by acetic acid. Alkaline earth metal salt solubilities are also reliant on hydration energy. Acetic acid reacts chemically with oxides, carbonates, and hydroxides but not with oxalates because it is an acid.