What is the approximate concentration of free Cu+ ion at equilibrium when1.91x10-2 mol copper(I) nitrate is added to 1.00 L of solution that is 1.030 Min CN. For [Cu(CN)₂], K = 1.0x1024.[Cut] =Muse tine References to access important values ir needed for this question.What is the approximate concentration of free Cd2+ ion at equilibrium when1.48x10-2 mol cadmium(II) nitrate is added to 1.00 L of solution that is 1.030M in CN. For [Cd (CN)4]2, K₁= 6.0x10¹8.[Cd2+] =M

Answer:- This question is answered by using the simple concept of calculation of equilibrium…

What is the approximate concentration of free Cu+ ion at equilibrium when 1.91x10-2 mol copper(I) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cu(CN)₂], K = 1.0x1024. [Cut] = M use ure References to access important values if needed for this question. What is the approximate concentration of free Cd2+ ion at equilibrium when 1.48x10-2 mol cadmium(II) nitrate is added to 1.00 L of solution that is 1.030 M in CN™. For [Cd (CN)4]2, K₁= 6.0x10¹8. [Cd²+] = M

What is the approximate concentration of free Cu+ ion at equilibrium when 1.91x10-2 mol copper(I) nitrate is added to 1.00 L of solution that is 1.030 M in CN. For [Cu(CN)₂], K = 1.0x1024. [Cut] = M use ure References to access important values if needed for this question. What is the approximate concentration of free Cd2+ ion at equilibrium when 1.48x10-2 mol cadmium(II) nitrate is added to 1.00 L of solution that is 1.030 M in CN™. For [Cd (CN)4]2, K₁= 6.0x10¹8. [Cd²+] = M

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter15: Solubility And Complex Lon Equilibria

Section: Chapter Questions

Problem 69E: A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 103 M CuNO3. Assume that...

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A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 103 M CuNO3. Assume that Cu+ forms complex ions with X as follows: Cu+(aq)+X(aq)CuX(aq)K1=1.0102CuX(aq)+X(aq)CuX2(aq)K2=1.0104CuX2(aq)+X(aq)CuX32(aq)K3=1.0103 with an overall reaction Cu+(aq)+3X(aq)CuX32(aq)K=1.0109 Calculate the following concentrations at equilibrium. a. Cux32 b. CuX2 c. Cu+
The Kf for the dicyanosilver complex ion, [Ag(CN)2]-, is 5.6 x 1018. When solid NaCN is added to a 0.010 M solution of AgNO3, 0.50 M CN- was found to be present at equilibrium. Calculate the concentration of silver ion also present at equilibrium.
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