**Educational Text Transcription:**12. The \( K_{sp} \) for silver carbonate is \( 8.4 \times 10^{-12} \). The concentration of carbonate ions in a saturated solution is \( 1.28 \times 10^{-4} \) 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?\[ 2 \text{ HI(g)} \rightleftharpoons \text{H}_2\text{(g)} + \text{I}_2\text{(g)} \quad K_c = 0.016 \, @ \, 800 \, \text{K} \]14. Calculate the pH and pOH for each of the following solutions at 25°C: 1. \( 1.0 \times 10^{-3} \, \text{M} \, \text{OH}^- \) 2. 3. 4. 5. \( 1.0 \, \text{M} \, \text{H}^+ \) 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 \( 1.1 \times 10^{-10} \).

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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

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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**Educational Text Transcription:**

12. The \( K_{sp} \) for silver carbonate is \( 8.4 \times 10^{-12} \). The concentration of carbonate ions in a saturated solution is \( 1.28 \times 10^{-4} \) 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?

\[ 2 \text{ HI(g)} \rightleftharpoons \text{H}_2\text{(g)} + \text{I}_2\text{(g)} \quad K_c = 0.016 \, @ \, 800 \, \text{K} \]

14. Calculate the pH and pOH for each of the following solutions at 25°C:
1. \( 1.0 \times 10^{-3} \, \text{M} \, \text{OH}^- \)
2.
3.
4.
5. \( 1.0 \, \text{M} \, \text{H}^+ \)
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 \( 1.1 \times 10^{-10} \).

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