= 1.6 x 10-10Given the reactions below, calculate the molar solubility of AgCl (s) in 0.566 M NH3 (aq) at 25 degrees C.AgCl (s) →> Ag+ (aq) + Cl¯ (aq) KspAg+ (aq) + 2 NH3 (aq) →>Ag (NH3)+(aq) K = 1.7 x 107f2Report your answer rounded to two significant figures and do NOT include units. Use "e" for scientific notation. For example, 1.0 x10-14 is 1.0e-14.

Step 1: Step 2:There is 0.566 instead of 0.655 by mistake I solved this acc to 0.655 ... Hope you…

Answered: = 1.6 x 10-10 Given the reactions…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 44PS

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Calculate the equilibrium concentration of Ag*(aq) in a solution that is initially 0.140 M AgNO3 and 0.980 MNH3, and in which the following reaction takes place: Ag*(aq) + 2NH3(aq)= Ag(NH3);(ag) (Kf = 1.70×107)
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