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:CoCl4^2-(aq) <--> Co2+(aq) + 4Cl-(aq)We can conclude that:1. This reaction is:A. ExothermicB. EndothermicC. NeutralD. More information is needed to answer this question.2. When the temperature is decreased the equilibrium constant, K:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.3. When the temperature is decreased the equilibrium concentration of Co2+:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.
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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+(...
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