You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of
a. Are there any beakers where you would observe solid still present? How do you know?
b. Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations.
c. For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2-, compare? (You don't need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer.
d. Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need?
e. Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information?
f. How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?
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Step by Step Answer:
Chapter # 17- Solubility and Complex-Ion Equilibria
Section: Review Questions
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Question Posted: March 01, 2016 04:57:38