How do the concentrations of Ag^+ and CrO4^2- in a saturated solution above 1.0 g of solid Ag2 C

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How do the concentrations of Ag^+ and CrO4^2- in a saturated...

How do the concentrations of $\mathrm{Ag}^{+}$ and $\mathrm{CrO}_{4}^{2-}$ in a saturated solution above 1.0 $\mathrm{g}$ of solid $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ change when 100 $\mathrm{g}$ of solid $\mathrm{Ag}_{2} \mathrm{CrO}_{4}$ is added to the system? Explain.

Key Concepts

Saturated Solution

A saturated solution is one in which the maximum amount of solute has been dissolved in the solvent, and any additional solute remains undissolved. In such a system, there is a dynamic equilibrium between the dissolving solute and the undissolved solid, meaning that even though the processes of dissolution and precipitation continue, the concentrations of the dissolved ions remain constant.

Solubility Product (Ksp)

The solubility product is a constant, specific to a given sparingly soluble salt, that quantifies the equilibrium between the solid phase and its ions in solution. It is expressed as the product of the concentrations of the constituent ions, each raised to the power of their stoichiometric coefficients. The Ksp value remains fixed at a given temperature, meaning that in a saturated solution, the ion concentrations are determined solely by this value.

Chemical Equilibrium

Chemical equilibrium in the context of solubility refers to a state where the forward process of the solid dissolving into its ions and the reverse process of the ions precipitating back into the solid occur at the same rate. This balance ensures that the concentration of ions in the saturated solution stays constant as long as external conditions (like temperature) remain unchanged.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, it will shift in the direction that minimizes that disturbance. In the case of a saturated solution, adding more solid does not affect the established equilibrium because the solution already contains the maximum concentration of ions allowed by the Ksp, so the excess solid simply remains undissolved.

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