Open Question
Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZnCO3, (b) ZnS, (c) BiI3, (d) AgCN, (e) Ba3(PO4)2?
Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 66
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.)
Verified step by step guidance1
Identify the relevant equilibrium reactions: The dissolution of NiC2O4 and the formation of the complex ion with NH3. Write the balanced chemical equations for these reactions.
Write the expression for the solubility product constant (K_{sp}) for NiC2O4. This will involve the concentrations of Ni^{2+} and C2O4^{2-} ions.
Write the expression for the formation constant (K_f) for the complex ion [Ni(NH3)_6]^{2+}. This involves the concentration of Ni^{2+} and NH3.
Set up the equilibrium expressions for both the dissolution and complex formation reactions. Use the stoichiometry of the reactions to relate the concentrations of the species involved.
Combine the expressions for K_{sp} and K_f to solve for the concentration of NH3 required to dissolve 0.020 mol of NiC2O4 in 1.00 L of solution.
Related Practice
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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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
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
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?