What is the [Ag*] in a saturated solution of Ag₂SO4 in 0.20 M Na₂SO₂? Use the Data Tables to find the appropriate equilibrium constant. A. 7.8 x 10-5 M B. 7.7 x 103 M C. 3.3 × 10 M D.2.1 x 10-3 M E.4.2 x 103 M Solubility is a time where we get to use an ICE table! We will not include Ag₂SO4 in our equilibrium calculation because [Select] .The Ksp of Ag₂SO4 is equal to [Select] A82SO4(s) + SO4²- (aq) OM I 0.20 M *X C [Select] [Select] E We can plug in our E row to our Ksp formula and solve for x. Its value is [Select] M. From there, we get our final answer of [Select] 2 Ag²+ (aq)
What is the [Ag*] in a saturated solution of Ag₂SO4 in 0.20 M Na₂SO₂? Use the Data Tables to find the appropriate equilibrium constant. A. 7.8 x 10-5 M B. 7.7 x 103 M C. 3.3 × 10 M D.2.1 x 10-3 M E.4.2 x 103 M Solubility is a time where we get to use an ICE table! We will not include Ag₂SO4 in our equilibrium calculation because [Select] .The Ksp of Ag₂SO4 is equal to [Select] A82SO4(s) + SO4²- (aq) OM I 0.20 M *X C [Select] [Select] E We can plug in our E row to our Ksp formula and solve for x. Its value is [Select] M. From there, we get our final answer of [Select] 2 Ag²+ (aq)
General Chemistry - Standalone book (MindTap Course List)
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Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.97QP: A saturated solution of copper(II) iodate in pure water has a copper-ion concentration of 2.7 103...
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Question
![Here is a solubility question!
What is the [Ag*] in a saturated solution of Ag₂SO4 in 0.20 M Na₂SO4? Use the Data Tables to find the
appropriate equilibrium constant.
A. 7.8 x 10-5 M
B. 7.7 x 10-3 M
C. 3.3 x 10-6 M
D.2.1 x 10-3 M
E. 4.2 x 10-³ M
Solubility is a time where we get to use an ICE table! We will not include Ag₂SO4 in our
equilibrium calculation because
[Select]
The Ksp of Ag2SO4 is equal to
[Select]
A82SO4(s)
+ SO4²- (aq)
OM
0.20 M
+2x
+X
E
[Select]
[Select]
We can plug in our E row to our Ksp formula and solve for x. Its value is
[Select]
M. From there, we get our final answer of
[Select]
I
C
2 Ag²+ (aq)
V
V
>
>
>](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff01b8cd4-7ccd-4d5d-8713-a82b8783858b%2F369d2621-685b-4c40-af98-9225b0d221f1%2F4mqhxts_processed.png&w=3840&q=75)
Transcribed Image Text:Here is a solubility question!
What is the [Ag*] in a saturated solution of Ag₂SO4 in 0.20 M Na₂SO4? Use the Data Tables to find the
appropriate equilibrium constant.
A. 7.8 x 10-5 M
B. 7.7 x 10-3 M
C. 3.3 x 10-6 M
D.2.1 x 10-3 M
E. 4.2 x 10-³ M
Solubility is a time where we get to use an ICE table! We will not include Ag₂SO4 in our
equilibrium calculation because
[Select]
The Ksp of Ag2SO4 is equal to
[Select]
A82SO4(s)
+ SO4²- (aq)
OM
0.20 M
+2x
+X
E
[Select]
[Select]
We can plug in our E row to our Ksp formula and solve for x. Its value is
[Select]
M. From there, we get our final answer of
[Select]
I
C
2 Ag²+ (aq)
V
V
>
>
>
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