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.
887
views
Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 68
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)
Verified step by step guidance1
Identify the relevant equilibrium reactions and their constants: (1) Ag2S (s) ⇌ 2 Ag^+ (aq) + S^2- (aq) with Ksp, (2) H2S (aq) ⇌ H^+ (aq) + HS^- (aq) with Ka1, (3) HS^- (aq) ⇌ H^+ (aq) + S^2- (aq) with Ka2, and (4) Ag^+ (aq) + 2 Cl^- (aq) ⇌ AgCl2^- (aq) with Kf.
Write the expression for the equilibrium constant of the target reaction: K_target = [AgCl2^-]^2 [H2S] / ([Cl^-]^4 [H^+]^2).
Express the equilibrium constant for the target reaction in terms of the given constants: K_target = (Ksp * Kf^2) / (Ka1 * Ka2).
Substitute the given values of Ksp, Ka1, Ka2, and Kf into the expression for K_target.
Simplify the expression to find the numerical value of the equilibrium constant for the target reaction.
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.)
Open Question
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.
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)].
1107
views
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?
505
views
1
comments