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Calculate the concentration of Cu²+(aq) in a solution that contains 0.020 mol of CuCl, and 0.100 mol of NaCN in 1.0 L. Cu²*(aq) + 4 CN¯(aq) 2Cu(CN);¯(aq) K = 2.0 × 1030 (Hint: Do not overlook the reaction of CN¯ with water to give HCN.)

Calculate the concentration of Cu²+(aq) in a solution that contains 0.020 mol of CuCl, and 0.100 mol of NaCN in 1.0 L. Cu²*(aq) + 4 CN¯(aq) 2Cu(CN);¯(aq) K = 2.0 × 1030 (Hint: Do not overlook the reaction of CN¯ with water to give HCN.)

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculate the concentration of Cu²+(aq) in a solution that contains 0.020 mol of CuCl, and 0.100 mol of NaCN in 1.0 L. Cu²*(aq) + 4 CN¯(aq) 2Cu(CN);¯(aq) K = 2.0 × 1030 (Hint: Do not overlook the reaction of CN¯ with water to give HCN.)
Transcribed Image Text:Calculate the concentration of Cu²+(aq) in a solution that contains 0.020 mol of CuCl, and 0.100 mol of NaCN in 1.0 L. Cu²*(aq) + 4 CN¯(aq) 2Cu(CN);¯(aq) K = 2.0 × 1030 (Hint: Do not overlook the reaction of CN¯ with water to give HCN.)
Expert Solution
Step 1

                                                   Cu(aq)2+  + 4CN(aq)-   ⇌  Cu(CN)4(aq)2- 

Initially                                   0.020 mol      0.100 mol                    0

Change                                   -0.01999        -0.08                     +0.02

Equilibrium                        y M(negligible)     0.100-0.08 M               0.02 M

                                                                      0.02 M

K = [Cu(CN)42-][Cu2+][CN-]4  

2.0 x 1030  = 0.02y x (0.02)4 

y = 0.022.0 x 1030 x (0.02)4  = 6.25 x 10-26  M

   

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