Textbook Question
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. (Ka = 3.5 x 10^-4)
(a) 4.11
(b) 3.82
(c) 3.46
(d) 3.09
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Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 12
What is the solubility-constant expression for Ca3(PO4)2 (s)? (a) [Ca2+]3 [PO43-]2 (b) [Ca2+]3 [PO43-]2 / [Ca3(PO4)2] (c) [Ca(PO4)2] / [Ca2+]3 [PO43-]2 (d) [Ca2+]2 [PO43-]3
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Solubility Product Constant (Ksp)
The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. For a compound like Ca3(PO4)2, Ksp helps predict how much of the solid can dissolve in water.
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01:47
Solubility Product Constant
Dissociation of Ionic Compounds
When ionic compounds dissolve in water, they dissociate into their constituent ions. For calcium phosphate, Ca3(PO4)2, the dissociation can be represented as Ca3(PO4)2 (s) ⇌ 3 Ca2+ (aq) + 2 PO4^3- (aq). Understanding this dissociation is crucial for writing the correct Ksp expression, as it directly relates to the concentrations of the ions in solution.
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02:11Ionic Compounds Naming
Equilibrium Expressions
Equilibrium expressions are mathematical representations of the concentrations of reactants and products at equilibrium. For Ksp, the expression is formed by taking the concentrations of the ions produced from the dissolution of the solid, raised to their respective stoichiometric coefficients. This concept is essential for determining the correct form of the Ksp expression for any given ionic compound.
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Related Practice
Textbook Question
What is the pH of a buffer solution prepared by dissolving 0.250 mol of NaH2PO4 and 0.075 mol of NaOH in enough water to make 1.00 L of solution? (Ka (H2PO4-) = 6.2 X 10^-8)
(a) 6.32
(b) 6.83
(c) 7.21
(d) 7.71
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Textbook Question
The pH titration curve applies to the titration of 40.0 mL of a 0.100 M solution of an acid with 0.100 M NaOH. What are the approximate pKa values for this acid?
(a) pKa1 = 5, pKa2 = 10
(b) pKa1 = 7, pKa2 = 11
(c) pKa1 = 5, pKa2 = 10, pKa3 = 13
(d) pKa1 = 5, pKa2 = 7, pKa3 = 10
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Textbook Question
What is the molar solubility of BaF2 in a solution containing 0.0750 M LiF (Ksp = 1.7 x 10^-6)
(a) 2.3 x 10^-5 M
(b) 3.0 x 10^-4 M
(c) 1.2 x 10^-2 M
(d) 1.3 x 10^-3 M
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Textbook Question
What is the molar solubility of AgI in 0.20 M NaCN?
(a) 6.2 x 10^-4 M
(b) 1.0 x 10^-1 M
(c) 7.6 x 10^-2 M
(d) 2.1 x 10^-3 M
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Textbook Question
A solution containing sulfide ions is added to a solution of 0.036 M Cu2+ and 0.044 M Fe2+. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate?
(a) 1.4 x 10^-16 M, FeS
(b) 3.6 x 10^-35 M, CuS
(c) 3.6 x 10^-35 M, FeS
(d) 1.4 x 10^-16 M, C
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