Solution X 100 mL of 0.10 M HCI Solution Y 200 mL of 0.50 M NAOH Solution Z 300 mL of distilled water Show work! A student prepares three solutions, X, Y, and Z, as described in the table above. All solutions are measured at 25°C. (a) Using the information above, rank the solutions in order of increasing pH. (b) Which of the 3 solutions would have the greatest change in pH by the addition of 100 mL of distilled water? Justify your answer.

Solution X 100 mL of 0.10 M HCI Solution Y 200 mL of 0.50 M NAOH Solution Z 300 mL of distilled water Show work! A student prepares three solutions, X, Y, and Z, as described in the table above. All solutions are measured at 25°C. (a) Using the information above, rank the solutions in order of increasing pH. (b) Which of the 3 solutions would have the greatest change in pH by the addition of 100 mL of distilled water? Justify your answer.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 38QAP: . Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar...

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What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
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A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Consider two weak acids, HA (MM=138g/mol)and HB (MM=72.0g/mol). A solution consisting of 11.0 g of HA in 745 mL has the same pH as a solution made up of 5.00 g of HB in 525 mL. Which of the two acids is stronger? Justify your answer by an appropriate calculation.
A solution of baking soda, NaHCO3, has a pH of 10.08. What is the percent (by mass) of NaHCO3 in a 235-mL solution? (Assume a density of 1.00 g/mL.)
. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
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