The final product of this reaction, [Cu(NH3)4]SO4 H₂O is soluble in water. What will you add to the solution after you add the concentrated ammonia to cause this product to precipitate out of solution? O 95% ethanol methanol isopropyl alcohol Nothing will be added. The precipitate will form when the solution is cooled in an ice bath. O Nothing will be added. The precipitate that we will isolate will form as the concentrated NH3 is added to the solution of [Cu(H₂O)4]2+

The final product of this reaction, [Cu(NH3)4]SO4 H₂O is soluble in water. What will you add to the solution after you add the concentrated ammonia to cause this product to precipitate out of solution? O 95% ethanol methanol isopropyl alcohol Nothing will be added. The precipitate will form when the solution is cooled in an ice bath. O Nothing will be added. The precipitate that we will isolate will form as the concentrated NH3 is added to the solution of [Cu(H₂O)4]2+

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

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 80E: The solubility of copper(II) hydroxide in water can be increased by adding either the base NH3 or...

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My Notes Write the solubility product reaction and the equilibrium constant expression, Ksp, for CaF2(s)
In Reaction 2, you added silver nitrate (AgNO3) to your solution of 1.0 M CoCl2. As mentioned in the lab procedure, silver nitrate dissociates in solution, yielding Ag+ and NO3-. Silver I (Ag+) loves chloride ions and will strongly bind to any that it can find. Upon binding with the chloride ions, a precipitate forms. Using your lab data to help you, answer the following questions below. Co(H2O)6^2+ (aq) + 4 Cl- <---> CoCl4^2- (aq) + 6H20(I) (Pink) (blue) Immediately following the addition of AgNO3 to your reaction: The value of Kc will be (less than/more than/equal) Qc. Equilibrium will shift to (Favor reactant/favor prodcut) . After AgNO3 is added, the color of the cobalt solution will be ( more pink/more blue/same color)
TWO SEPERATE QUESTIONS, REVIEW BOTH IMAGES
A solution containing cobalt (I) ions is added to a solution that is 0.034 M Br– and 0.069 M Cl–. What is the identity of the precipitate that forms, and at what concentration of cobalt (I) ions does this begin to occur? Solubility Product Constants: CoCl = 2.1 × 10–5 CoBr = 6.2 × 10–12 No precipitate will form at any concentration of cobalt (I). CoCl, 9.0 × 10–11 M CoBr, 3.0 × 10–4 M CoCl, 6.2 × 10–4 M CoBr, 1.8 × 10–10 M
A 25.0 mL aqueous solution of 0.150 mol L-1 Co3+(aq) was prepared. To this solution, 0.0500 mol of NH3 is added. What is the concentration of Co3+ once equilibrium is reached at 25⁰C? (Kf([CO(NH3)6]3+) = 2.3 × 1033) a. 3.7 × 10-35 mol L-1 b. 8.9 × 10-33 mol L-1 c. 4.6 × 10-32 mol L-1 d. 1.1 × 10-38 mol L-1 e. 4.9× 10-34 mol L-1
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