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Kw = 5.48 × 10-¹4 at 50 °C. A solution is prepared by dissolving 0.030 mol of Ba(OH)2 in 1.50 L of aqueous solution at 50 °C. What is the pH of this solution? A. 12.60 B. 11.86 C. 12.30 D. 11.56 E. 11.04

Kw = 5.48 × 10-¹4 at 50 °C. A solution is prepared by dissolving 0.030 mol of Ba(OH)2 in 1.50 L of aqueous solution at 50 °C. What is the pH of this solution? A. 12.60 B. 11.86 C. 12.30 D. 11.56 E. 11.04

Chemistry
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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Answer: B
**Problem:** At 50°C, the ion product of water, \( K_w \), is \( 5.48 \times 10^{-14} \). A solution is prepared by dissolving 0.030 mol of \( \text{Ba(OH)}_2 \) in 1.50 L of aqueous solution at 50°C. What is the pH of this solution? **Options:** A. 12.60 B. 11.86 C. 12.30 D. 11.56 E. 11.04 This problem involves calculating the pH of a solution containing a strong base, barium hydroxide (\( \text{Ba(OH)}_2 \)), at a specific temperature. The challenge is to determine how the dissolved barium hydroxide contributes hydroxide ions (\( \text{OH}^- \)) to the solution, and hence, find the pH.
Transcribed Image Text:**Problem:** At 50°C, the ion product of water, \( K_w \), is \( 5.48 \times 10^{-14} \). A solution is prepared by dissolving 0.030 mol of \( \text{Ba(OH)}_2 \) in 1.50 L of aqueous solution at 50°C. What is the pH of this solution? **Options:** A. 12.60 B. 11.86 C. 12.30 D. 11.56 E. 11.04 This problem involves calculating the pH of a solution containing a strong base, barium hydroxide (\( \text{Ba(OH)}_2 \)), at a specific temperature. The challenge is to determine how the dissolved barium hydroxide contributes hydroxide ions (\( \text{OH}^- \)) to the solution, and hence, find the pH.
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