A student prepares an acetic acid/sodium acetate buffer by mixing 10.00 mL of 0.50 M acetic acid with 0.4102 g of sodium acetate. This buffer is then tested by adding 0.10 M HCI and 0.10 M NaOH, and the following data is obtained: 0.10 M HCI added 0.10 M NaOH added Buffer Volume (mL) 40.00 40.00 Amount of Acid/Base Added (ml) 17.06 18.71 Initial pH 4.75 4.75 Final pH 3.72 3: Calculate the buffer capacity for both the acid and base additions. 5.78 1: Calculate the concentration of acetic acid and acetate ion in the buffer. Considering these concentrations, what is significant about the initial pH of 4.75? 2: Which component (Acetic acid or Acetate ion) reacts with HCI? Which component (Acetic acid or Acetate ion) reacts with NaOH? Write the balanced neutralization reaction for both.

A student prepares an acetic acid/sodium acetate buffer by mixing 10.00 mL of 0.50 M acetic acid with 0.4102 g of sodium acetate. This buffer is then tested by adding 0.10 M HCI and 0.10 M NaOH, and the following data is obtained: 0.10 M HCI added 0.10 M NaOH added Buffer Volume (mL) 40.00 40.00 Amount of Acid/Base Added (ml) 17.06 18.71 Initial pH 4.75 4.75 Final pH 3.72 3: Calculate the buffer capacity for both the acid and base additions. 5.78 1: Calculate the concentration of acetic acid and acetate ion in the buffer. Considering these concentrations, what is significant about the initial pH of 4.75? 2: Which component (Acetic acid or Acetate ion) reacts with HCI? Which component (Acetic acid or Acetate ion) reacts with NaOH? Write the balanced neutralization reaction for both.

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 34QAP: A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of...

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A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Calculate the solubility of AgCN in moles per liter and grams per liter. Ksp for AgCN is 6.0 1017.
Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0 mL of 0.10 M HCl. a. What color is the solution initially? b. The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow) occur? c. What color will the solution be after 200.0 mL NaOH has been added?
A buffer is made up of 239 mL of 0.187 M potassium hydrogen tartrate (KHC4H4O6) and 137 mL of 0.288 M potassium tartrate (K2C4H4O6). Ka for is (H2C4H4O6)4.55105. Assuming volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after adding 0.0250 mol of HCI to 0.376 L of the buffer. (c) the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer.