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Ch.17 - Applications of Aqueous Equilibria
All textbooksMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblem 14
Chapter 17, Problem 14

Consider a saturated solution of the slightly soluble salt BaCO3. Adding which of the following substances will increase the solubility? (a) HNO3 (b) Na2CO3 (c) Ba(NO3)2 (d) KOH

Verified step by step guidance
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Step 1: Understand the concept of solubility and the common ion effect. The solubility of a salt in solution can be affected by the presence of other ions that either share a common ion with the salt or react with the ions of the salt.
Step 2: Consider the effect of adding HNO3. Adding an acid like HNO3 can increase the solubility of BaCO3 by reacting with the carbonate ions (CO3^2-) to form carbonic acid (H2CO3), which further decomposes into CO2 and H2O, thus removing CO3^2- ions from the solution.
Step 3: Analyze the effect of adding Na2CO3. Adding Na2CO3 will increase the concentration of CO3^2- ions in the solution, which will shift the equilibrium towards the formation of more solid BaCO3, thus decreasing its solubility due to the common ion effect.
Step 4: Evaluate the impact of adding Ba(NO3)2. Adding Ba(NO3)2 will increase the concentration of Ba^2+ ions in the solution, which will also shift the equilibrium towards the formation of more solid BaCO3, decreasing its solubility due to the common ion effect.
Step 5: Consider the effect of adding KOH. Adding KOH will increase the pH of the solution, but it does not directly affect the solubility of BaCO3 since it does not remove CO3^2- ions or add a common ion.

Key Concepts

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

Saturation and Solubility Product (Ksp)

A saturated solution is one where the maximum amount of solute has dissolved at a given temperature, and any additional solute will not dissolve. The solubility product constant (Ksp) quantifies the equilibrium between the solid and its ions in solution. For BaCO3, the Ksp expression is [Ba^2+][CO3^2-], and changes in ion concentrations can shift this equilibrium, affecting solubility.
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Solubility Product Constant

Common Ion Effect

The common ion effect describes how the solubility of a salt decreases in the presence of a common ion. For BaCO3, adding a source of either Ba^2+ or CO3^2- ions will shift the equilibrium to the left, reducing solubility. Understanding this effect is crucial for predicting how different substances will influence the solubility of BaCO3 in solution.
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Common Ion Effect

Acid-Base Reactions and Solubility

Acids can increase the solubility of certain salts by reacting with their anions. In the case of BaCO3, adding HNO3 introduces H+ ions, which can react with CO3^2- to form HCO3^- or H2CO3, effectively removing CO3^2- from the solution. This shift can increase the solubility of BaCO3 by reducing the concentration of the common ion.
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Related Practice
Textbook Question
The pH titration curve applies to the titration of 40.0 mL of a 0.100 M solution of an acid with 0.100 M NaOH. What are the approximate pKa values for this acid?

(a) pKa1 = 5, pKa2 = 10(b) pKa1 = 7, pKa2 = 11(c) pKa1 = 5, pKa2 = 10, pKa3 = 13 (d) pKa1 = 5, pKa2 = 7, pKa3 = 10
Textbook Question
What is the solubility-constant expression for Ca3(PO4)2 (s)? (a) [Ca2+]3 [PO43-]2(b) [Ca2+]3 [PO43-]2 / [Ca3(PO4)2](c) [Ca(PO4)2] / [Ca2+]3 [PO43-]2(d) [Ca2+]2 [PO43-]3
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What is the molar solubility of BaF2 in a solution containing 0.0750 M LiF (Ksp = 1.7 x 10^-6)(a) 2.3 x 10^-5 M(b) 3.0 x 10^-4 M(c) 1.2 x 10^-2 M(d) 1.3 x 10^-3 M
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