Slaked lime, Ca(OH)2, is used to soften hard water by...

Slaked lime, $\mathrm{Ca}(\mathrm{OH})_{2}$, is used to soften hard water by removing calcium ions from hard water through the reaction $\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{Ca}^{2+}(a q)+2 \mathrm{HCO}_{3}^{-}(a q) \rightarrow$ Although $\mathrm{CaCO}_{3}(s)$ is considered insoluble, some of it does dissolve in aqueous solutions. Calculate the molar solubility of $\mathrm{CaCO}_{3}$ in water $\left(K_{\mathrm{sp}}=8.7 \times 10^{-9}\right)$

Slaked lime, $\mathrm{Ca}(\mathrm{OH})_{2}$, is used to soften hard water by removing calcium ions from hard water through the reaction
$\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{Ca}^{2+}(a q)+2 \mathrm{HCO}_{3}^{-}(a q) \rightarrow$
Although $\mathrm{CaCO}_{3}(s)$ is considered insoluble, some of it does dissolve in aqueous solutions. Calculate the molar solubility of $\mathrm{CaCO}_{3}$ in water $\left(K_{\mathrm{sp}}=8.7 \times 10^{-9}\right)$

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Key Concepts

Molar Solubility

Molar solubility is defined as the number of moles of a solute that can dissolve in one liter of a solvent to form a saturated solution. It directly relates to the Ksp through the stoichiometry of the dissolution reaction, allowing for the calculation of the concentrations of the ions in solution at equilibrium.

Solubility Product Constant (Ksp)

The solubility product constant, or Ksp, is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It represents the product of the molar concentrations of the ions each raised to the power of their respective coefficients in the dissolution reaction when the solution is saturated. This constant is crucial for predicting the solubility of ionic compounds and determining whether precipitation will occur in a given solution.

Dissolution Equilibrium

Dissolution equilibrium refers to the state reached when a sparingly soluble salt dissolves in a solvent until the rate of dissolution equals the rate of precipitation. This dynamic equilibrium is described by the solubility product constant and is fundamental to understanding how changes in concentration, temperature, or common ions can affect the solubility of a compound.

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