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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 90a
Capitolo 17, Problema 90a

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08⨉10-5 M

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Identify the dissolution equation for BaCrO_4: BaCrO_4(s) \(\rightleftharpoons\) Ba^{2+}(aq) + CrO_4^{2-}(aq).
Recognize that the molar solubility of BaCrO_4 is given as 1.08 \(\times\) 10^{-5} M, which means [Ba^{2+}] = 1.08 \(\times\) 10^{-5} M and [CrO_4^{2-}] = 1.08 \(\times\) 10^{-5} M at equilibrium.
Write the expression for the solubility product constant (K_{sp}): K_{sp} = [Ba^{2+}][CrO_4^{2-}].
Substitute the equilibrium concentrations into the K_{sp} expression: K_{sp} = (1.08 \(\times\) 10^{-5})(1.08 \(\times\) 10^{-5}).
Calculate the value of K_{sp} by multiplying the concentrations.

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Molar Solubility

Molar solubility is the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (M). It provides a quantitative measure of how much of a compound can be present in solution before reaching saturation. Understanding molar solubility is essential for calculating the solubility product constant (Ksp) of sparingly soluble salts.
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Molar Solubility Example

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. Ksp provides insight into the extent to which a compound can dissolve in water and is crucial for predicting precipitation reactions.
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Solubility Product Constant

Dissolution Equilibrium

Dissolution equilibrium refers to the dynamic balance between the solid phase of a solute and its ions in solution. For a compound like BaCrO4, the dissolution can be represented by a chemical equation where the solid dissociates into its constituent ions. At equilibrium, the rate of dissolution equals the rate of precipitation, allowing for the calculation of Ksp based on the concentrations of the ions in solution.
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Thermal Equilibrium
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