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Ch.17 - Additional Aspects of Aqueous Equilibria
All textbooksBrown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblem 69
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Chapter 17, Problem 69

(a) Will Ca(OH)2 precipitate from solution if the pH of a 0.050 M solution of CaCl2 is adjusted to 8.0? (b) Will Ag2SO4 precipitate when 100 mL of 0.050 M AgNO3 is mixed with 10 mL of 5.0 * 10^-2 M Na2SO4 solution?

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1
Step 1: Determine the solubility product constant (K_sp) for Ca(OH)_2 and Ag_2SO_4 from a reliable source or textbook.
Step 2: For part (a), calculate the concentration of OH^- ions at pH 8.0 using the formula [OH^-] = 10^{-(14 - pH)}.
Step 3: Calculate the ion product (Q) for Ca(OH)_2 using the formula Q = [Ca^{2+}][OH^-]^2, where [Ca^{2+}] is given as 0.050 M.
Step 4: Compare the ion product (Q) with the solubility product constant (K_sp) for Ca(OH)_2. If Q > K_sp, precipitation will occur.
Step 5: For part (b), calculate the concentrations of Ag^+ and SO_4^{2-} ions after mixing the solutions, then calculate the ion product (Q) for Ag_2SO_4 and compare it with its K_sp to determine if precipitation occurs.
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Related Practice
Open Question
From the value of Kf listed in Table 17.1, calculate the concentration of NH3 required to just dissolve 0.020 mol of NiC2O4 (Ksp = 4 * 10^-102) in 1.00 L of solution? (Hint: You can neglect the hydrolysis of C2O4^2- because the solution will be quite basic.)
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Use values of Ksp for AgI and Kf for [Ag(CN)2]- to (a) calculate the molar solubility of AgI in pure water. (b) calculate the equilibrium constant for the reaction AgI(s) + 2 CN⁻(aq) ⇌ [Ag(CN)2]⁻(aq) + I⁻(aq). (c) determine the molar solubility of AgI in a 0.100 M NaCN solution.
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Using the value of Ksp for Ag2S, Ka1 and Ka2 for H2S, and Kf = 1.1 * 10^5 for AgCl2^-, calculate the equilibrium constant for the following reaction: Ag2S (s) + 4 Cl^- (aq) + 2 H^+ (aq) ⇌ 2 AgCl2^- (aq) + H2S (aq)
Textbook Question

Calculate the minimum pH needed to precipitate Mn1OH22 so completely that the concentration of Mn2 +1aq2 is less than 1 mg per liter [1 part per billion (ppb)].

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Textbook Question

Suppose that a 10-mL sample of a solution is to be tested for I- ion by addition of 1 drop (0.2 mL) of 0.10 M Pb1NO322. What is the minimum number of grams of I- that must be present for PbI21s2 to form?

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Open Question
A solution contains 2.0 * 10^-4 M Ag^+ (aq) and 1.5 * 10^-3 M Pb^2+ (aq). If NaI is added, will AgI (Ksp = 8.3 * 10^-17) or PbI2 (Ksp = 7.9 * 10^-9) precipitate first? Specify the concentration of I^- (aq) needed to begin precipitation.