1. A solid weak acid is dissolved in water. Half of the solution is titrated to the end point with NaOH solution, using phenolphthalein as indicator. To the other half is added an equivalent amount of H₂O to keep the volume identical. The neutralized and acid solutions are then mixed and the pH of the resulting solution is found to be 4.20. Find the Ka of the solid acid. 2. Is it acceptable to pour NaOH solution from the stock bottle directly into a clamped buret? YES OR NO. (Circle the correct answer) 3.50.00 mL of a solution of HNO₂ (Ka = 3.98x104) is combined with 50.00 mL of a solution of NaNO₂ to create a pH buffer solution. The pH of the buffer solution is found to be 4.00. a. What is the ratio of NO₂: HNO2 in the buffer described above? b. What ratio of NO2: HNO2 would be necessary to establish a buffer with a pH of 2.80?

1. A solid weak acid is dissolved in water. Half of the solution is titrated to the end point with NaOH solution, using phenolphthalein as indicator. To the other half is added an equivalent amount of H₂O to keep the volume identical. The neutralized and acid solutions are then mixed and the pH of the resulting solution is found to be 4.20. Find the Ka of the solid acid. 2. Is it acceptable to pour NaOH solution from the stock bottle directly into a clamped buret? YES OR NO. (Circle the correct answer) 3.50.00 mL of a solution of HNO₂ (Ka = 3.98x104) is combined with 50.00 mL of a solution of NaNO₂ to create a pH buffer solution. The pH of the buffer solution is found to be 4.00. a. What is the ratio of NO₂: HNO2 in the buffer described above? b. What ratio of NO2: HNO2 would be necessary to establish a buffer with a pH of 2.80?

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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