Open Question
Calculate the molar solubility of SrF2 in: (a) 0.010 M Sr(NO3)2 (b) 0.010 M NaF.
Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 115
Consider saturated solutions of the slightly soluble salt AgBr. Is the solubility of AgBr increased, decreased, or unaffected by the addition of each of the following substances? (a) HBr, (b) HNO3, (c) AgNO3, (d) NH3.
Verified step by step guidance1
Step 1: Understand the concept of solubility equilibrium. AgBr is a slightly soluble salt, and its solubility can be represented by the equilibrium: AgBr(s) ⇌ Ag⁺(aq) + Br⁻(aq). The solubility product constant (Ksp) governs this equilibrium.
Step 2: Analyze the effect of adding HBr. HBr is a strong acid that dissociates completely in water to give H⁺ and Br⁻ ions. Adding HBr increases the concentration of Br⁻ ions, which shifts the equilibrium to the left according to Le Chatelier's principle, decreasing the solubility of AgBr.
Step 3: Consider the addition of HNO3. HNO3 is a strong acid that dissociates to give H⁺ and NO₃⁻ ions. Since neither of these ions directly affects the Ag⁺ or Br⁻ ions in the solubility equilibrium, the solubility of AgBr is unaffected by HNO3.
Step 4: Evaluate the effect of adding AgNO3. AgNO3 dissociates to give Ag⁺ and NO₃⁻ ions. The increase in Ag⁺ ion concentration shifts the equilibrium to the left, decreasing the solubility of AgBr due to the common ion effect.
Step 5: Assess the impact of adding NH3. NH3 can react with Ag⁺ ions to form a complex ion, [Ag(NH3)2]⁺, which reduces the concentration of free Ag⁺ ions. This shifts the equilibrium to the right, increasing the solubility of AgBr.
Related Practice
Open Question
Which of the following compounds are more soluble in an acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction: (b) CaCO3, (c) Ni(OH)2, (d) Ca3(PO4)2.
Textbook Question
Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (b) Fe(OH)3
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Open Question
Consider saturated solutions of the slightly soluble salt BaCO3. Is the solubility of BaCO3 increased, decreased, or unaffected by the addition of each of the following substances? (a) HNO3 (b) Ba(NO3)2 (c) Na2CO3 (d) CH3CO2H
Textbook Question
Is the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (a) HCl
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Textbook Question
Is the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (b) KOH