Bundle: Chemistry for Engineering Students, Loose-Leaf Version, 4th + OWLv2 with MindTap Reader with Student Solutions Manual, 1 term (6 months) Printed Access Card

4th Edition

ISBN: 9780357000403

Author: Lawrence S. Brown, Tom Holme

Publisher: Cengage Learning

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Textbook Question

Chapter 12, Problem 12.41PAE

Because calcium carbonate is a sink for CO₃²- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is

Ca²⁺(aq) + COj²^_(aq) ** CaCO,(s)

The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions?

A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake:

H₂COj(aq) H⁺(aq) + HCO_}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?

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Chapter 12, Problem 12.40PAE

Chapter 12, Problem 12.42PAE

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Chapter 12 Solutions

Bundle: Chemistry for Engineering Students, Loose-Leaf Version, 4th + OWLv2 with MindTap Reader with Student Solutions Manual, 1 term (6 months) Printed Access Card

Ch. 12 - list chemical reactions important in the...Ch. 12 - Explain that equilibrium is dynamic, and that at...Ch. 12 - Prob. 3CO Ch. 12 - calculate equilibrium constants from experimental...Ch. 12 - Prob. 5CO Ch. 12 - calculate molar solubility from Kspor vice versa.Ch. 12 - Prob. 7CO Ch. 12 - Prob. 8CO Ch. 12 - calculate the new equilibrium composition of a...Ch. 12 - Explain the importance of both kinetic and...

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Solution Summary: The author explains that the equilibrium concentration of ions should be calculated for the following reaction.

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Chapter 12 Solutions