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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.18 - Aqueous Ionic EquilibriumProblem 95a
Chapter 18, Problem 95a

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M

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Identify the dissolution equation for the compound MX: MX(s) \(\rightleftharpoons\) M^+(aq) + X^-(aq).
Recognize that the molar solubility of MX is given as 3.27 \(\times\) 10^{-11} M, which means [M^+] = [X^-] = 3.27 \(\times\) 10^{-11} M at equilibrium.
Write the expression for the solubility product constant (K_{sp}): K_{sp} = [M^+][X^-].
Substitute the equilibrium concentrations into the K_{sp} expression: K_{sp} = (3.27 \(\times\) 10^{-11})(3.27 \(\times\) 10^{-11}).
Calculate the K_{sp} value by multiplying the concentrations.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Solubility

Molar solubility is the number of moles of a solute that can dissolve in a liter of solvent at a given temperature, expressed in moles per liter (M). It provides a quantitative measure of how much of a compound can dissolve to form a saturated solution. Understanding molar solubility is essential for calculating the solubility product constant (Ksp) of ionic compounds.
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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that reflects the extent to which a sparingly soluble ionic compound dissolves in water. It is calculated from the concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced dissolution equation. Ksp values are crucial for predicting the solubility of compounds and understanding precipitation reactions.
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Dissociation of Ionic Compounds

When ionic compounds dissolve in water, they dissociate into their constituent ions. For example, a compound MX will dissociate into M⁺ and X⁻ ions. The stoichiometry of this dissociation is important for calculating Ksp, as the concentrations of the ions produced directly influence the Ksp value. Understanding this process is vital for accurately determining the solubility product from molar solubility.
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