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Ch.17 - Applications of Aqueous Equilibria
All textbooksMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblem 14
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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
1
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.
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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
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Textbook Question
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