12. The Ksp for silver carbonate is 8.4 x 1012. Theconcentration of carbonate ions in a saturated solution1.28 x 10 4 M. What is the concentration of silver ions?13. 4.00 moles of HI are placed in an evacuated 5.00 Lflask and then heated to 800 K. The system is allowed toreach equilibrium. What will be the equilibriumconcentration of each species? (2 HI(g) H2(g) + 12(g) Kc = 0.016 @ 800 K14. Calculate the pH and pOH for each of the followingsolutions at 25°C.1. 1.0x 10-3 M OH-2.3.4.5. 1.0M H +6.7.8.15. Estimate the solubility of barium sulfate in a 0.020 Msodium sulfate solution. The solubility product constantfor barium sulfate is 1.1 x 10-10.

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Answered: 12. The Ksp for silver carbonate is 8.4…

12. The Ksp for silver carbonate is 8.4 x 1012. The concentration of carbonate ions in a saturated solution is 1.28 x 10 4 M. What is the concentration of silver ions?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.98PAE

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Question

12. The Ksp for silver carbonate is 8.4 x 1012. The
concentration of carbonate ions in a saturated solution
1.28 x 10 4 M. What is the concentration of silver ions?
13. 4.00 moles of HI are placed in an evacuated 5.00 L
flask and then heated to 800 K. The system is allowed to
reach equilibrium. What will be the equilibrium
concentration of each species? (
2 HI(g) H2(g) + 12(g) Kc = 0.016 @ 800 K
14. Calculate the pH and pOH for each of the following
solutions at 25°C.
1. 1.0x 10-3 M OH-
2.
3.
4.
5. 1.0M H +
6.
7.
8.
15. Estimate the solubility of barium sulfate in a 0.020 M
sodium sulfate solution. The solubility product constant
for barium sulfate is 1.1 x 10-10.

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