1. A student doing the experiment in this module extended the study of the [COCI,Pion/Co(H₂O) ion equilibrium. In one test tube, the student added silver nitrate (AgNO,) to a blue equilibrium mixture prepared from CoCl₂. The reaction mixture became pink and cloudy, and a white precipitate settled out leaving a clear, pink solution. The student identified the precipitate as silver chloride, AgCl. (1) Briefly explain how these observations are consistent with Le Châtelier's principle. In a second test, the student placed a test tube containing a pink equilibrium mixture in a hot-water bath. The solution turned blue. When the student removed the test tube from the hot-water bath and placed it in an ice-water bath, the solution turned pink. (2) Is the forward reaction in the ICOCI, ion/Co(H₂O), ion equilibrium exothermic or endothermic? (3) Briefly explain how the student's observations support your answer to (2). (4) Write the net ionic equation for this equilibrium, including heat.
1. A student doing the experiment in this module extended the study of the [COCI,Pion/Co(H₂O) ion equilibrium. In one test tube, the student added silver nitrate (AgNO,) to a blue equilibrium mixture prepared from CoCl₂. The reaction mixture became pink and cloudy, and a white precipitate settled out leaving a clear, pink solution. The student identified the precipitate as silver chloride, AgCl. (1) Briefly explain how these observations are consistent with Le Châtelier's principle. In a second test, the student placed a test tube containing a pink equilibrium mixture in a hot-water bath. The solution turned blue. When the student removed the test tube from the hot-water bath and placed it in an ice-water bath, the solution turned pink. (2) Is the forward reaction in the ICOCI, ion/Co(H₂O), ion equilibrium exothermic or endothermic? (3) Briefly explain how the student's observations support your answer to (2). (4) Write the net ionic equation for this equilibrium, including heat.
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please answer each question. Note that each question has 3 or 4 sub-part
Transcribed Image Text:1. A student doing the experiment in this module extended the study of the [CoC1,2-ion/[Co(H₂O),1²+
ion equilibrium. In one test tube, the student added silver nitrate (AgNO,) to a blue equilibrium
mixture prepared from CoCl₂. The reaction mixture became pink and cloudy, and a white precipitate
settled out leaving a clear, pink solution. The student identified the precipitate as silver chloride,
AgCl.
(1) Briefly explain how these observations are consistent with Le Châtelier's principle.
In a second test, the student placed a test tube containing a pink equilibrium mixture in a hot-water
bath. The solution turned blue. When the student removed the test tube from the hot-water bath and
placed it in an ice-water bath, the solution turned pink.
(2) Is the forward reaction in the [CoC, ion/[Co(H₂O), ion equilibrium exothermic or
endothermic?
(3) Briefly explain how the student's observations support your answer to (2).
(4) Write the net ionic equation for this equilibrium, including heat.
Transcribed Image Text:2. The popular antacid, Milk of Magnesia, is a suspension of magnesium hydroxide, Mg(OH)2. In water,
Mg(OH)₂ undergoes the reaction shown in Equation 9.
Mg(OH)₂ (s, white) = Mg²+ (aq) + 2OH(aq)
(Eq. 9)
(1) What would you observe if you added an acid to an equilibrium mixture containing Mg(OH)₂ in
water?
(2) Write a chemical equation that accounts for the effect of the added acid.
(3) Briefly explain how your answer to (1) is consistent with Le Châtelier's principle.
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