Cobalt(II) complex ion solution: [Co(H2O)6]*2(aq) + 4CI'(aq) [COC14] ?(aq) + 6H2O(I) Pink Blue (3) According to the first video (a) What will happen when HCl is added ? That is in which direction the equilibrium shifts and the conc of which cobalt compound increases and which one decreases ? (b) What will happen if instead of HCI , CaCl, is added ? (c) What will happen when water is added to test tube (1) ? That is in which direction the equilibrium shifts and the conc of which cobalt compound increases and which one decreases ?

Cobalt(II) complex ion solution: [Co(H2O)6]*2(aq) + 4CI'(aq) [COC14] ?(aq) + 6H2O(I) Pink Blue (3) According to the first video (a) What will happen when HCl is added ? That is in which direction the equilibrium shifts and the conc of which cobalt compound increases and which one decreases ? (b) What will happen if instead of HCI , CaCl, is added ? (c) What will happen when water is added to test tube (1) ? That is in which direction the equilibrium shifts and the conc of which cobalt compound increases and which one decreases ?

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 formation constant Kf for the complex ion Zn(OH)4^2- is 2.8 X10^15 . What is the concentration of zinc ion, Zn2+ , in a solution that is initially 0.47 M in Zn(OH)4^2-? [Zn2+] =______ M
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When AgCl(s) is dissolved in a solution of NH3, the complex ion Ag(NH3)2+ forms as shown in the following reaction. AgCl(s)+2NH3⇌Ag(NH3)2+(aq)+Cl−(aq), KC=2.4×10−3 If the Ksp of AgCl is 1.6 × 10–10, what is the Kf for Ag(NH3)2+?
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addition of 0.10M sodium chloride and 0.10M ammonia to a 0.10M silver nitrate solution. KSP = 1.77 × 10-10, KF = 1.7 × 10-7 Calculate Q for the concentrations given. use Q and compare to K, which of precipitate or complex ion will happen?
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