The equation below shows the equilibrium that exists between the two ions of copper. A mixture of the two lons has an intermediate blue-green color. Cu(H₂O) (aq) + 4C (aq) CuCl(aq) + 4H₂O(1) blue yellow Predict what color the mixture above will have as a result of the following changes in the space provided below indicate your prediction and explain why the resulting colors appear. [Explanations must be specific and relate to concepts learned in this class) Al Sodium chloride (NaCl) is added to the mixture, b Water is added to the mixture.

The equation below shows the equilibrium that exists between the two ions of copper. A mixture of the two lons has an intermediate blue-green color. Cu(H₂O) (aq) + 4C (aq) CuCl(aq) + 4H₂O(1) blue yellow Predict what color the mixture above will have as a result of the following changes in the space provided below indicate your prediction and explain why the resulting colors appear. [Explanations must be specific and relate to concepts learned in this class) Al Sodium chloride (NaCl) is added to the mixture, b Water is added to the mixture.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 93AE: Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72 , and the yellow...

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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.
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl². 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: Co²+ (aq) + 4C1 (aq) = CoCl₂² (aq) We can conclude that: 1. This reaction O exothermic. O endothermic. Oneutral. O More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: O increases. Odecreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co²+: O increases. Odecreases. O remains the same. OMore information is needed to answer this question. Previc
The blue complex Cu(H,O);+ and the yellow complex CuCl- exist in equilibrium. Cu(H, O);+(aq) + 4 CI¯(aq) = CuCl (aq) + 4 H, O(1) Upon addition of LiCl to this equilibrium in solution, which observation would be expected? The solution turns blue. The solution turns yellow. The Cu2+ salts precipitate out of solution. The volume of water decreases. Incorrect O O O
The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe (aq) + SCN (aq) = Fe(SCN)²+* (aq) increasing the concentration of Fe³+ decreasing the concentration of Fe(SCN)²+ increasing the temperature of the system Answer Bank about us carten privacy polic terms of use contact us help
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
Consider the following equilibrium system: Ag+(aq) + 2NH3(aq) D Ag(NH3)2+(aq) + energy If the equilibrium concentrations are as follows, what is the value of Keq? [Ag+] = 2.0M , [NH3] = 6.0 M , [Ag(NH3)2+] = 8.0M
Cobalt(ll) chloride can form two complexes when dissolved in water [Co(H 2 O) 6 )^ 2 + (aq) which is pink in colour, and [CoCl 4 ]^ 2- (ac) which is blue. The equilibrium system [CO(H 2 O) 6 ]^ 2 +(aq)(pink)+4 Cl^ - (aq) doubleheaded arrow [CoCl 4 )^ 2- (aq)(blue)+ 6H 2 O(l) (a) Describe how the system and its colour will change in each of the following situations (I) HCL is added (II) water is added (III) AgNO 3 is added if an aqueous solution of cobalt(II)chloride placed in a hot water bath at 90 Celsius,the solution will turn blue . If the solution is placed in an ice salt mixture , it will turn pink. Is the reaction as written above exothermic or endothermic ? Explain your reasoning
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
The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe3+(aq) ++ SCN−(aq) ↽−−⇀↽−−⇀ Fe(SCN)2+(aq) increasing the concentration of Fe3+ decreasing the concentration of Fe(SCN)2 increasing the temperature of the system Answer Bank ↑↑ ↓↓
Calcium hydroxide will precipitate from solution by the following equilibrium: 2+ Ca²+ (aq) + 2OH(aq) + Ca(OH)₂ (s) Write the equilibrium expression for this reaction.
Scott prepares a solution which contains a large excess of iron and a small amount of thiocyanate. He notices a faint orange color appear in the solution once mixed. He repeats this process with a higher concentration of thiocyanate and notices a deepening of the orange color in the solution once mixed. Explain what has happened to the equilibrium in this case. Has the value of Keq changed? Explain.
(a) In the determination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in mg/L., on the basis of the solubility product principle, when the chloride concentration has been reduced to 0.2 mg/L? (b) If the concentration of chromate indicator used is 5 x 10 M, how much excess silver ion in mg/L. must be present before the formation of a red precipitate will begin?

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