At Low Temperature the pink color predominates. At High Temperature the blue color is strong. COC1,?(aq) fwe represent the equilibrium as: Co2*(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of Co2+: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
At Low Temperature the pink color predominates. At High Temperature the blue color is strong. COC1,?(aq) fwe represent the equilibrium as: Co2*(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of Co2+: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
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Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.103QP: Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia....
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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+(aq) is pink and CoCl42-(aq) is blue.
... At Low Temperature the pink color predominates. ... |
... At High Temperature the blue color is strong. ... |
If we represent the equilibrium as:...Co2+(aq) + 4Cl-(aq) CoCl42-(aq)
We can conclude that:
| fill in the blank 1 | 1. | This reaction is: |
| A. Exothermic | ||
| B. Endothermic | ||
| C. Neutral | ||
| D. More information is needed to answer this question. | ||
fill in the blank 2 |
2. | When the temperature is decreased the equilibrium constant, K: |
| A. Increases | ||
| B. Decreases | ||
| C. Remains the same | ||
| D. More information is needed to answer this question. | ||
fill in the blank 3 |
3. | When the temperature is decreased the equilibrium concentration of Co2+: |
| A. Increases | ||
| B. Decreases | ||
| C. Remains the same | ||
| D. More information is needed to answer this question. |
Transcribed Image Text:In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl,2. Co2"(aq) is pink and CoCl,2 (aq) is blue.
At Low Temperature the pink color predominates.
At High Temperature the blue color is strong.
If we represent the equilibrium as: Co2*(aq) + 4CI(aq)
2
COCI, (aq)
We can conclude that:
1. This reaction is:
A. Exothermic
B. Endothermic
C. Neutral
D. More information is needed to answer this question.
2. When the temperature is decreased the equilibrium constant, K:
A. Increases
B. Decreases
C. Remains the same
D. More information is needed to answer this question.
O 3. When the temperature is decreased the equilibrium concentration of Co2*:
A. Increases
B. Decreases
C. Remains the same
Previous
Next
D. More information is needed to answer this question.
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