(Solved): im am totally lost  In an aqueous chloride solution cobalt(II) exists in equilibrium with the c ...

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion \( \mathrm{CoCl}_{4}{ }^{2-} \). \( \mathrm{Co}^{2+}(a q) \) is pink and \( \mathrm{CoCl}_{4}{ }^{2-}(a q) \) is blue. \( \begin{array}{ll}\text { At low ............ predominates. } & \text { At high temperature the blue color is } \\ \text { strong. }\end{array} \) If we represent the equilibrium as: \[ \mathrm{CoCl}_{4}{ }^{2-}(a q) \rightleftharpoons \mathrm{Co}^{2+}(a q)+4 \mathrm{Cl}^{-}(a q) \] \[ \mathrm{CoCl}_{4}^{2-}(a q) \rightleftharpoons \mathrm{Co}^{2+}(a q)+4 \mathrm{Cl}^{-}(a q) \] ean 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. More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of \( \mathrm{CoCl}_{4}{ }^{2 .} \) increases. decreases. remains the same. More information is needed to answer this question. No more group attempts remain