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For a 0.09 M solution of HBr, calculate: [H3O+], pH, pOH, and [OH-] Make sure to enter all answers to three decimal places. Enter 1.234x10-5 as 1.234e-5 H3O+ = 0.09 ? <✓100% pH = 1.05 pOH = 12.95 [OH-] = 1.122e-13 ? ✓ 100% C. ? ✓ 100% Now make the same calculations for a 1.35e-11 M solution of HCl H3O+ = 4.95 pH = 10.87 pOH = 3.13 [OH-] = 4.47e-10 2. ? ✓ 100% ? × 0% ? × 0% ? × 0% C. ? × 0%

For a 0.09 M solution of HBr, calculate: [H3O+], pH, pOH, and [OH-] Make sure to enter all answers to three decimal places. Enter 1.234x10-5 as 1.234e-5 H3O+ = 0.09 ? <✓100% pH = 1.05 pOH = 12.95 [OH-] = 1.122e-13 ? ✓ 100% C. ? ✓ 100% Now make the same calculations for a 1.35e-11 M solution of HCl H3O+ = 4.95 pH = 10.87 pOH = 3.13 [OH-] = 4.47e-10 2. ? ✓ 100% ? × 0% ? × 0% ? × 0% C. ? × 0%

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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For a 0.09 M solution of HBr, calculate: [H3O+], pH, pOH, and [OH-] Make sure to enter all answers to three decimal places. Enter 1.234x10-5 as 1.234e-5 H3O+ = 0.09 ? <✓100% pH = 1.05 pOH = 12.95 [OH-] = 1.122e-13 ? ✓ 100% C. ? ✓ 100% Now make the same calculations for a 1.35e-11 M solution of HCl H3O+ = 4.95 pH = 10.87 pOH = 3.13 [OH-] = 4.47e-10 2. ? ✓ 100% ? × 0% ? × 0% ? × 0% C. ? × 0%
Transcribed Image Text:For a 0.09 M solution of HBr, calculate: [H3O+], pH, pOH, and [OH-] Make sure to enter all answers to three decimal places. Enter 1.234x10-5 as 1.234e-5 H3O+ = 0.09 ? <✓100% pH = 1.05 pOH = 12.95 [OH-] = 1.122e-13 ? ✓ 100% C. ? ✓ 100% Now make the same calculations for a 1.35e-11 M solution of HCl H3O+ = 4.95 pH = 10.87 pOH = 3.13 [OH-] = 4.47e-10 2. ? ✓ 100% ? × 0% ? × 0% ? × 0% C. ? × 0%
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