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solve and show work In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42Co2+(aq) is pink and CoCl42(aq) is blue. At
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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42Co2+(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: 1. This reaction is exothermic. endothermic. neutral. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K : increases. decreases. remains the same. Co2+(aq)+4Cl(aq)CoCl42(aq) conclude that: 1. This reaction is exothermic. endothermic. neutral. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, I increases. decreases. remains the same. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentratio increases. decreases. remains the same. More information is needed to answer this Step by Step Solution
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