"If AgCl(s) is in equilibrium with dissolved AgCl according to the following equation: AgCl(s) <-> Ag+(aq) + Cl-(aq) If the equilibrium constant for this process is: Kc = -1.8*10-10, what is the Ag+ concentration when AgCl is dissolved in pure water?"
"If AgCl(s) is in equilibrium with dissolved AgCl according to the following equation: AgCl(s) <-> Ag+(aq) + Cl-(aq) If the equilibrium constant for this process is: Kc = -1.8*10-10, what is the Ag+ concentration when AgCl is dissolved in pure water?"
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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Stuck on a practice test problem.
"If AgCl(s) is in equilibrium with dissolved AgCl according to the following equation:
AgCl(s) <-> Ag+(aq) + Cl-(aq)
If the equilibrium constant for this process is: Kc = -1.8*10-10, what is the Ag+ concentration when AgCl is dissolved in pure water?"
A. 1.3*10-5
B. 2.8*10-5
C. 3.6*10-10
D. 9.0*10-11
E. 5.5*10-6
The answer key says it is A, but I am unsure of how to get there.
Any explanation on where to start would be greatly appreciated!
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