762 CHAPTER 17 Additional Aspects of Aqueous Equilibria 17.55 A 1.00-L solution saturated at 25 °C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide contains 0.54 g of Pbl2. Calculate the solubility-product constant for this salt at 25 °C. 17.57 Using Appendix D, calculate the molar solubility of AgBr in (a) pure water, (b) 3.0 × 10 2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.58 Calculate the solubility of LaF3 in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF, in equilibrium with undissolved CaF2(s). Solid CaCl, is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca²+ ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 7.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? .61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. -62 Calculate the molar golul 'i

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
icon
Related questions
icon
Concept explainers
Question

56

762
CHAPTER 17 Additional Aspects of Aqueous Equilibria
17.55 A 1.00-L solution saturated at 25 °C with calcium oxalate
(CaC2O4) contains 0.0061 g of CaC2O4. Calculate the
solubility-product constant for this salt at 25 °C.
17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide
contains 0.54 g of Pbl2. Calculate the solubility-product
constant for this salt at 25 °C.
17.57 Using Appendix D, calculate the molar solubility of AgBr in
(a) pure water, (b) 3.0 × 10 2 M AgNO3 solution, (c) 0.10 M
NaBr solution.
17.58 Calculate the solubility of LaF3 in grams per liter in (a) pure
water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution.
17.59 Consider a beaker containing a saturated solution of CaF,
in equilibrium with undissolved CaF2(s). Solid CaCl, is
then added to the solution. (a) Will the amount of solid
CaF, at the bottom of the beaker increase, decrease, or re-
main the same? (b) Will the concentration of Ca²+ ions in
solution increase or decrease? (c) Will the concentration of
F ions in solution increase or decrease?
7.60 Consider a beaker containing a saturated solution of PbI2
in equilibrium with undissolved PbI2(s). Now solid KI is
added to this solution. (a) Will the amount of solid Pbl2 at
the bottom of the beaker increase, decrease, or remain the
same? (b) Will the concentration of Pb2+ ions in solution
increase or decrease? (c) Will the concentration of I ions
in solution increase or decrease?
.61 Calculate the solubility of Mn(OH)2 in grams per liter
when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8.
-62 Calculate the molar golul 'i
Transcribed Image Text:762 CHAPTER 17 Additional Aspects of Aqueous Equilibria 17.55 A 1.00-L solution saturated at 25 °C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide contains 0.54 g of Pbl2. Calculate the solubility-product constant for this salt at 25 °C. 17.57 Using Appendix D, calculate the molar solubility of AgBr in (a) pure water, (b) 3.0 × 10 2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.58 Calculate the solubility of LaF3 in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF, in equilibrium with undissolved CaF2(s). Solid CaCl, is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca²+ ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 7.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? .61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. -62 Calculate the molar golul 'i
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 4 images

Blurred answer
Knowledge Booster
Lipids
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY