Textbook Question
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (d) Hg2C2O4.
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Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 67
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.
Verified step by step guidance1
Step 1: Identify the relevant equilibrium expressions. For AgI, the solubility product (K_{sp}) is given by the expression: K_{sp} = [Ag^+][I^-]. For the complex ion formation, the formation constant (K_f) is given by: K_f = \frac{[Ag(CN)_2^-]}{[Ag^+][CN^-]^2}.
Step 2: Calculate the molar solubility of AgI in pure water. Assume the solubility of AgI is 's' mol/L. Then, [Ag^+] = s and [I^-] = s. Substitute these into the K_{sp} expression to solve for 's'.
Step 3: Write the overall reaction for the dissolution of AgI in the presence of CN^-: AgI(s) + 2 CN^- \rightleftharpoons [Ag(CN)_2]^- + I^-. The equilibrium constant for this reaction (K_{overall}) can be found by multiplying K_{sp} and K_f.
Step 4: Calculate the molar solubility of AgI in a 0.100 M NaCN solution. Assume the solubility of AgI is 's' mol/L. In this case, [CN^-] is approximately 0.100 M. Use the expression for K_{overall} to solve for 's', considering the initial concentration of CN^-.
Step 5: Set up the equilibrium expression for the reaction in the NaCN solution: K_{overall} = \frac{[Ag(CN)_2^-][I^-]}{[CN^-]^2}. Substitute the known values and solve for the molar solubility 's'.
Related Practice
Textbook Question
From the value of Kf listed in Table 17.1, calculate the concentration of Ni2 +1aq2 and Ni1NH326 2+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH31aq2.
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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.)
Open Question
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)
Open Question
(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?
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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