General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN: 9781305580343

Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher: Cengage Learning

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Textbook Question

Chapter 17, Problem 17.15QP

Solubility 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 don’t 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?

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Chapter 17, Problem 17.14QP

Chapter 17, Problem 17.16QP

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125.0 mL of a solution of iron (III) nitrate and 125.0 mL of a solution of ammonium dichromate get mixed into a large beaker. Some precipitate forms which is collected and found to weigh 24.93 grams. The concentration of dichromate ions was measured after the reaction took place and found to be 0.4713 M. Answer the following questions regarding this reaction D)Using your balanced molecular reaction set up an ICE Chart and fill in the End (or final) mole values for every reactant and product and then the change and initial rows as well for every reactant and product.

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Chapter 17 Solutions

General Chemistry - Standalone book (MindTap Course List)

Ch. 17.1 - Give solubility product expressions for the...Ch. 17.1 - Silver ion may be recovered from used photographic...Ch. 17.1 - Lead(II) arsenate, Pb3(AsO4)2, has been used as an...Ch. 17.1 - Prob. 17.4E Ch. 17.1 - Prob. 17.1CC Ch. 17.2 - a. Calculate the molar solubility of barium...Ch. 17.2 - Suppose you have equal volumes of saturated...Ch. 17.2 - Prob. 17.3CC Ch. 17.3 - Anhydrite is a mineral composed of CaSO4 (calcium...Ch. 17.3 - A solution of 0.00016 M lead(II) nitrate,...

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