Ascorbic acid is a diprotic acid with pKa1 = 4.l and pK2 = 11.8. You have an ascorbate buffer with pH 11.2. What is the buffer range of this buffer? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 10.2 to 12.2 b 3.1 to 5.1 10.8 to 12.8 10.7 to 11.7 11.3 to 12.3

Ascorbic acid is a diprotic acid with pKa1 = 4.l and pK2 = 11.8. You have an ascorbate buffer with pH 11.2. What is the buffer range of this buffer? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 10.2 to 12.2 b 3.1 to 5.1 10.8 to 12.8 10.7 to 11.7 11.3 to 12.3

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 32QAP: Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate...

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Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
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Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 M
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.