In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL42. Co²+ (aq) is pink and CoC14²(aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: CoC14²(aq) Co²+ (aq) + 4Cl¯ (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of CoC₁4²: O increases. O decreases. O remains the same. O More information is needed to answer this question.
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL42. Co²+ (aq) is pink and CoC14²(aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: CoC14²(aq) Co²+ (aq) + 4Cl¯ (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of CoC₁4²: O increases. O decreases. O remains the same. O More information is needed to answer this question.
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 98CWP
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Transcribed Image Text:In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL42. Co²+ (aq) is pink and CoC14²(aq) is blue.
At low temperature the pink color predominates. At high temperature the blue color is strong.
If we represent the equilibrium as:
CoC14²(aq) Co²+ (aq) + 4Cl¯ (aq)
We can conclude that:
1. This reaction is
O exothermic.
O endothermic.
O neutral.
O More information is needed to answer this question.
2. When the temperature is decreased the equilibrium constant, K:
O increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
3. When the temperature is decreased the equilibrium concentration of CoC₁4²:
O increases.
O decreases.
O remains the same.
O More information is needed to answer this question.
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