2 a) Calculate the concentration of Zn+2 in a0.01 M solution of Zn(NO3)2 and containingan added NH3 concentration of 3.2x102 M.We have the complex ion formation constantsof: Zn(NH3)+2 kl = 151, Zn(NH3)2+2; k2 = 178,Zn(NH3)3*2; k3 = 204, Zn(NH3)4+2 ; k4 = 91.2+2.b) If 1.2 x 10-10 M of Sulfide ions (S<) areadded to the previous solution, will the ZnSprecipitate? (for SnS Kps = 1 x 10-24)

Zn2+ + 4NH3 ⇌ [Zn(NH3)42+] It is the overall reaction equation.Now, moles of Zn = 0.01As per the…

a) Calculate the concentration of Zn+2 in a 0.01 M solution of Zn(NO3)2 and containing an added NH3 concentration of 3.2x10-2 M. We have the complex ion formation constants of: Zn(NH3) k1 = 151, Zn(NH3)2*2 ; k2 = 178, +2 %3D %3D

a) Calculate the concentration of Zn+2 in a 0.01 M solution of Zn(NO3)2 and containing an added NH3 concentration of 3.2x10-2 M. We have the complex ion formation constants of: Zn(NH3) k1 = 151, Zn(NH3)2*2 ; k2 = 178, +2 %3D %3D

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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