Solution X 100mL of 0.10M NaOH (aq) is mixed with 100mL of 0.10M HBr(aq) Solution Y 100mL of 0.1M NaBr(aq) is mixed with 100mL of 0.10M HBr(aq) Solution Z 100mL of 0.1 M HC2H3O2 (aq) is mixed with 100mL of 0.10M NaC2H3O2(aq) A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below. Species Ka HBr >>1(very large) HC2H3O2 1.8x10^-5 a. Using the information above, write the letters of the solutions to rank the solutions in order of increasing pH. Explain your reasoning for the ranking. Lowest pH Highest pH < < b.Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer. c.The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes much more than the pH of solution Z changes. Explain this observation.
Solution X 100mL of 0.10M NaOH (aq) is mixed with 100mL of 0.10M HBr(aq) Solution Y 100mL of 0.1M NaBr(aq) is mixed with 100mL of 0.10M HBr(aq) Solution Z 100mL of 0.1 M HC2H3O2 (aq) is mixed with 100mL of 0.10M NaC2H3O2(aq) A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below. Species Ka HBr >>1(very large) HC2H3O2 1.8x10^-5 a. Using the information above, write the letters of the solutions to rank the solutions in order of increasing pH. Explain your reasoning for the ranking. Lowest pH Highest pH < < b.Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer. c.The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes much more than the pH of solution Z changes. Explain this observation.
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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| Solution X | 100mL of 0.10M NaOH (aq) is mixed with 100mL of 0.10M HBr(aq) |
| Solution Y | 100mL of 0.1M NaBr(aq) is mixed with 100mL of 0.10M HBr(aq) |
| Solution Z | 100mL of 0.1 M HC2H3O2 (aq) is mixed with 100mL of 0.10M NaC2H3O2(aq) |
A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below.
| Species | Ka |
| HBr | >>1(very large) |
| HC2H3O2 | 1.8x10^-5 |
a. Using the information above, write the letters of the solutions to rank the solutions in order of increasing pH. Explain your reasoning for the ranking.
| Lowest pH | Highest pH | |
| < | < |
b.Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer.
c.The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes much more than the pH of solution Z changes. Explain this observation.
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