Consider the equilibrium that is established in a saturatedsolution of silver chloride, Ag+(aq) + Cl-(aq) ⇌ AgCl(s).If solid AgCl is added to this solution, what will happen tothe concentration of Ag+ and Cl- ions in solution?(a) [Ag+] and [Cl-] will both increase (b) [Ag+] and [Cl-] willboth decrease (c) [Ag+] will increase and [Cl-] will decrease(d) [Ag+] will decrease and [Cl-] will increase (e) neither [Ag+] nor [Cl-] will change
Consider the equilibrium that is established in a saturatedsolution of silver chloride, Ag+(aq) + Cl-(aq) ⇌ AgCl(s).If solid AgCl is added to this solution, what will happen tothe concentration of Ag+ and Cl- ions in solution?(a) [Ag+] and [Cl-] will both increase (b) [Ag+] and [Cl-] willboth decrease (c) [Ag+] will increase and [Cl-] will decrease(d) [Ag+] will decrease and [Cl-] will increase (e) neither [Ag+] nor [Cl-] will change
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...
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Consider the equilibrium that is established in a saturated
solution of silver chloride, Ag+(aq) + Cl-(aq) ⇌ AgCl(s).
If solid AgCl is added to this solution, what will happen to
the concentration of Ag+ and Cl- ions in solution?
(a) [Ag+] and [Cl-] will both increase (b) [Ag+] and [Cl-] will
both decrease (c) [Ag+] will increase and [Cl-] will decrease
(d) [Ag+] will decrease and [Cl-] will increase (e) neither
[Ag+] nor [Cl-] will change
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