Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Question
Chapter 14, Problem 14.72QE
Interpretation Introduction
Interpretation:
The solubility of
Concept Introduction:
Solubility product is the equilibrium constant for the reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by
The expression for its
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Chapter 14 Solutions
Chemistry: Principles and Practice
Ch. 14 - Prob. 14.1QECh. 14 - Describe a nonchemical system that is in...Ch. 14 - Describe a nonchemical system that is not in...Ch. 14 - Prob. 14.4QECh. 14 - Prob. 14.5QECh. 14 - Prob. 14.6QECh. 14 - Prob. 14.7QECh. 14 - Prob. 14.8QECh. 14 - Prob. 14.9QECh. 14 - Prob. 14.10QE
Ch. 14 - Explain why terms for pure liquids and solids do...Ch. 14 - Temperature influences solubility. Does...Ch. 14 - Prob. 14.13QECh. 14 - Prob. 14.14QECh. 14 - Prob. 14.15QECh. 14 - Prob. 14.16QECh. 14 - Prob. 14.17QECh. 14 - Prob. 14.18QECh. 14 - At 2000 K, experiments show that the equilibrium...Ch. 14 - At 500 K, the equilibrium constant is 155 for...Ch. 14 - At 77 C, Kp is 1.7 104 for the formation of...Ch. 14 - Consider the following equilibria involving SO2(g)...Ch. 14 - Kc at 137 C is 4.42 for NO(g) + 12 Br2(g) NOBr(g)...Ch. 14 - Prob. 14.24QECh. 14 - Prob. 14.25QECh. 14 - Prob. 14.26QECh. 14 - Prob. 14.27QECh. 14 - Prob. 14.28QECh. 14 - Prob. 14.29QECh. 14 - Prob. 14.30QECh. 14 - Prob. 14.31QECh. 14 - Prob. 14.32QECh. 14 - Prob. 14.33QECh. 14 - Prob. 14.34QECh. 14 - Prob. 14.35QECh. 14 - Consider the system...Ch. 14 - Prob. 14.37QECh. 14 - Prob. 14.38QECh. 14 - Prob. 14.39QECh. 14 - Prob. 14.40QECh. 14 - Prob. 14.41QECh. 14 - Prob. 14.42QECh. 14 - Prob. 14.43QECh. 14 - Prob. 14.44QECh. 14 - Prob. 14.45QECh. 14 - Prob. 14.46QECh. 14 - Prob. 14.47QECh. 14 - Prob. 14.48QECh. 14 - Prob. 14.49QECh. 14 - Prob. 14.50QECh. 14 - Prob. 14.51QECh. 14 - Consider 0.200 mol phosphorus pentachloride sealed...Ch. 14 - Prob. 14.53QECh. 14 - Prob. 14.54QECh. 14 - Prob. 14.55QECh. 14 - Prob. 14.56QECh. 14 - Prob. 14.57QECh. 14 - Prob. 14.58QECh. 14 - Prob. 14.59QECh. 14 - Prob. 14.60QECh. 14 - Prob. 14.61QECh. 14 - Write the expression for the equilibrium constant...Ch. 14 - Prob. 14.63QECh. 14 - Prob. 14.64QECh. 14 - Write the expression for the solubility product...Ch. 14 - Prob. 14.66QECh. 14 - Prob. 14.67QECh. 14 - The solubility of silver iodate, AgIO3, is 1.8 ...Ch. 14 - Prob. 14.69QECh. 14 - Prob. 14.70QECh. 14 - Prob. 14.71QECh. 14 - Prob. 14.72QECh. 14 - Even though barium is toxic, a suspension of...Ch. 14 - Lead poisoning has been a hazard for centuries....Ch. 14 - Calculate the solubility of barium sulfate (Ksp =...Ch. 14 - Calculate the solubility of copper(II) iodate,...Ch. 14 - Calculate the solubility of lead fluoride, PbF2...Ch. 14 - Calculate the solubility of zinc carbonate, ZnCO3...Ch. 14 - Prob. 14.79QECh. 14 - Prob. 14.80QECh. 14 - Use the solubility product constant from Appendix...Ch. 14 - Prob. 14.82QECh. 14 - Some barium chloride is added to a solution that...Ch. 14 - Prob. 14.84QECh. 14 - Prob. 14.85QECh. 14 - Prob. 14.86QECh. 14 - Prob. 14.87QECh. 14 - Prob. 14.88QECh. 14 - Prob. 14.89QECh. 14 - Prob. 14.90QECh. 14 - Prob. 14.91QECh. 14 - At 3000 K, carbon dioxide dissociates CO2(g) ...Ch. 14 - Prob. 14.94QECh. 14 - Nitrogen, hydrogen, and ammonia are in equilibrium...Ch. 14 - The concentration of barium in a saturated...Ch. 14 - According to the Resource Conservation and...Ch. 14 - Prob. 14.98QE
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- You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.arrow_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardWhen carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)arrow_forward
- Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72 , and the yellow chromate ion, CrO42 . (See the following photos.) The equilibrium reaction between the two ions is Cr2O72(aq)+H2O(l)2CrO42(aq)+2H+(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added.arrow_forwardCalculate the molarity of AgNO3 in a solution prepared by dissolving 1.44 g AgNO3 in enough water to form 1.00 L solution.arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forward
- Phosphate buffers are important in regulating the pH of intracellular fluids. If the concentration ratio of H2PO4/HPO42 in a sample of intracellular fluid is 1.1: 1, what is the pH of this sample of intracellular fluid? H2PO4(aq)HPO42(aq)+H+(aq)Ka=6.2108arrow_forwardThe solubility rules outlined in Chapter 4 say that Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH of a saturated solution of each of these marginally soluble hydroxides.arrow_forwardSolubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?arrow_forward
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