In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC14². 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: + (aq) + 4Cl¯¯(aq) ⇒ CoCl² (aq) Co²+ 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 Co²+: 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 CoC14². 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: + (aq) + 4Cl¯¯(aq) ⇒ CoCl² (aq) Co²+ 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 Co²+: O increases. O decreases. O remains the same. O More information is needed to answer this question.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 123QRT: You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3,...

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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoClą2-. 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: Coclą2 (aq) = 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 increased 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 increased the equilibrium concentration of Co2+: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
2+ In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC142. Co²+ (aq) is pink and CoCl2(aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: 2+ CoCl2(aq) Co²+ (aq) + 4C1¯ (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. Oneutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. decreases. remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of Co²+: Prev
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.
and the con 2. Given the following two reactions and their equilibrium constants: Cu(H,O),*(aq) + 4 NH3(aq) =Cu(NH3),²*(aq) + 4 H,O(1) K¡ = 5 × 102 Cu(H2O),?*(aq) + CO,²-=CUCO;(s) + 4 H,O(I) K, = 7 × 10° Evaluate the equilibrium constant for the reaction (see discussion): Cu(NH3),*(aq) + CO,²-(aq)= CUCO;(s) + 4 NH;(aq) b. When 1 M concentrations of all dissolved species are present, which is more stable, CuCO3 or Cu(NH,),*? Explain your reasoning. custom page
The preparation of cis-platin [Pt(NH 3) 2CI 2], an anticancer drug, uses an equilibrium reaction: K 2PECI 4(aq) + 2NH 3(aq) = 2 KCI(aq) + Pt(NH 3) 2CI 2(aq). Which of the following conditions would lead to an increase in the amount of Pt(NH 3) 2CI 2 formed? The use of a low concentration of NH3 The addition of a large concentration of KCI The use of a large concentration of NH3 The use of a stoichiometric ration of K2PTCI4 and NH3