Consider the insoluble compound aluminum phosphate , AlIPO4. The aluminum ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of AIPO, (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction, For Al(OH)4 , K= 7.7x1033. Use the pull-down boxes to specify states such as (aq) or (s). K = Consider the insoluble compound copper(II) hydroxide , Cu(OH), . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3),* , Kf= 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). 2 Cu(NH3), 2+ Cu(OH)2 + |4NH3 ( (aq) 3 / 2 Cu(NH,)"| (s) (aq) 20Н (aq) K= 1.36x10^-6 Incorrect Feedback: Partially Correct Incorrect Correct Answer(s): (s) in water and is the equation for the equilibrium in a saturated solution of Cu(OH)2 - The second step represems tne rormauon or me ammonia complex from the Cu2* ion in solution. As the Cu(NH3),* complex forms, Cu²* ion The first step below 1.1*10^-6 is removed from solution and the dissolution equilibrium shifts to the right. The sum of these two equations gives the desired equation, with an equilibrium constant given by the product of the K's for the first two. Cu(ОН)2 (8) 2 Cu²* (aq) + 2 OH" (aq) Кр — 1.6х10-19 Cu2* (aq) + 4 NH3 (aq) 2 Cu(NH3),* (aq) Kf= 6.8×1012 !! Cu(OH)2(s) + 4NH3(aq) 2 Cu(NH3),*(aq) + 20H°(aq) Knet = Kp X Kf=1.1×106 Note that Knet >> Ksp indicating a substantial increase in the solubility of Cu(OH), (s). (Previous Next
Consider the insoluble compound aluminum phosphate , AlIPO4. The aluminum ion also forms a complex with hydroxide ions . Write a balanced net ionic equation to show why the solubility of AIPO, (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction, For Al(OH)4 , K= 7.7x1033. Use the pull-down boxes to specify states such as (aq) or (s). K = Consider the insoluble compound copper(II) hydroxide , Cu(OH), . The copper(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Cu(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3),* , Kf= 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s). 2 Cu(NH3), 2+ Cu(OH)2 + |4NH3 ( (aq) 3 / 2 Cu(NH,)"| (s) (aq) 20Н (aq) K= 1.36x10^-6 Incorrect Feedback: Partially Correct Incorrect Correct Answer(s): (s) in water and is the equation for the equilibrium in a saturated solution of Cu(OH)2 - The second step represems tne rormauon or me ammonia complex from the Cu2* ion in solution. As the Cu(NH3),* complex forms, Cu²* ion The first step below 1.1*10^-6 is removed from solution and the dissolution equilibrium shifts to the right. The sum of these two equations gives the desired equation, with an equilibrium constant given by the product of the K's for the first two. Cu(ОН)2 (8) 2 Cu²* (aq) + 2 OH" (aq) Кр — 1.6х10-19 Cu2* (aq) + 4 NH3 (aq) 2 Cu(NH3),* (aq) Kf= 6.8×1012 !! Cu(OH)2(s) + 4NH3(aq) 2 Cu(NH3),*(aq) + 20H°(aq) Knet = Kp X Kf=1.1×106 Note that Knet >> Ksp indicating a substantial increase in the solubility of Cu(OH), (s). (Previous Next
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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Transcribed Image Text:Consider the insoluble compound aluminum phosphate , AlIPO4. The aluminum ion also forms a complex with hydroxide ions . Write a balanced net
ionic equation to show why the solubility of AIPO, (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this
reaction,
For Al(OH)4 , K= 7.7x1033. Use the pull-down boxes to specify states such as (aq) or (s).
K =
Transcribed Image Text:Consider the insoluble compound copper(II) hydroxide , Cu(OH), . The copper(II) ion also forms a complex with ammonia . Write a balanced net
ionic equation to show why the solubility of Cu(OH), (s) increases in the presence of ammonia and calculate the equilibrium constant for this
reaction.
For Cu(NH3),* , Kf= 6.8×1012 . Use the pull-down boxes to specify states such as (aq) or (s).
2 Cu(NH3),
2+
Cu(OH)2
+ |4NH3
( (aq) 3 / 2 Cu(NH,)"|
(s)
(aq)
20Н
(aq)
K= 1.36x10^-6
Incorrect
Feedback:
Partially Correct
Incorrect
Correct Answer(s):
(s) in water and is the equation for the equilibrium in a saturated solution of Cu(OH)2 -
The second step represems tne rormauon or me ammonia complex from the Cu2* ion in solution. As the Cu(NH3),* complex forms, Cu²* ion
The first step below 1.1*10^-6
is removed from solution and the dissolution equilibrium shifts to the right. The sum of these two equations gives the desired equation, with an
equilibrium constant given by the product of the K's for the first two.
Cu(ОН)2 (8)
2 Cu²* (aq) + 2 OH" (aq)
Кр — 1.6х10-19
Cu2* (aq) + 4 NH3 (aq)
2 Cu(NH3),* (aq)
Kf= 6.8×1012
!!
Cu(OH)2(s) + 4NH3(aq) 2 Cu(NH3),*(aq) + 20H°(aq)
Knet = Kp X Kf=1.1×106
Note that Knet >> Ksp indicating a substantial increase in the solubility of Cu(OH), (s).
(Previous
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