Si on introduit du chromate de potassium K2 CrO4 dans une solution saturée de sulfate d'argent A

step 1 we are asked to explain the situation I've written here. So, a couple things we need to know her

Si on introduit du chromate de potassium K2 CrO4 dans une...

$\mathrm{Si}$ on introduit du chromate de potassium $\mathrm{K}_2 \mathrm{CrO}_4$ dans une solution saturée de sulfate d'argent $\mathrm{Ag}_2 \mathrm{SO}_4$, contenant un excès de solide, ce dernier, qui est blanc, se transforme en un solide rouge constitué de chromate d'argent $\mathrm{Ag}_2 \mathrm{CrO}_4$. Comment peut-on expliquer ce changement de nature de la phase solide en équilibre avec la solution?

$\mathrm{Si}$ on introduit du chromate de potassium $\mathrm{K}_2 \mathrm{CrO}_4$ dans une solution saturée de sulfate d'argent $\mathrm{Ag}_2 \mathrm{SO}_4$, contenant un excès de solide, ce dernier, qui est blanc, se transforme en un solide rouge constitué de chromate d'argent $\mathrm{Ag}_2 \mathrm{CrO}_4$.
Comment peut-on expliquer ce changement de nature de la phase solide en équilibre avec la solution?

Key Concepts

Selective Precipitation

Selective precipitation involves manipulating solution conditions so that one compound with a lower solubility (and thus a lower Ksp) precipitates before another. By adding a reagent that introduces a new ion, the equilibrium can be shifted to favor the formation of one solid over another, as seen when a more insoluble salt replaces a less insoluble one in a saturated solution.

Le Chatelier's Principle

This principle states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance. In the context of solubility equilibria, adding an ion (or a compound producing that ion) can shift the equilibrium, leading to the precipitation of a less soluble compound to re-establish balance.

Solubility Equilibrium

This concept describes the balance between a sparingly soluble solid and its dissolved ions in solution. In a saturated solution, the rate at which the solid dissolves equals the rate at which ions precipitate, and the concentrations of the ions remain constant as long as the system is undisturbed.

Solubility Product (Ksp)

The solubility product is an equilibrium constant that represents the maximum product of the ionic concentrations in a saturated solution for a given salt. When the ionic product exceeds the Ksp, the excess ions will precipitate as a solid, indicating that the salt is less soluble under the given conditions.

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