You prepare a solution by mixing 100 mL of 0.1 M sodium acctate and 100 mL of 0.1 M acetic acid. You measure the pH and find that it is 4.8. 5. ,Could this solution function as a buffer? Explain (a) your answer. (b) When you measure the pH again, what will you observe? Explain your answer. You add 8 mL of 4 M NaOH to the solution.

You prepare a solution by mixing 100 mL of 0.1 M sodium acctate and 100 mL of 0.1 M acetic acid. You measure the pH and find that it is 4.8. 5. ,Could this solution function as a buffer? Explain (a) your answer. (b) When you measure the pH again, what will you observe? Explain your answer. You add 8 mL of 4 M NaOH to the solution.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 49P

See similar textbooks

Similar questions

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.
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
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)?
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.
Ka for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
weak acid = sodium bisulfate monohydrate, ?a=1.20×10−2,Ka=1.20×10−2, 3.00 M conjugate base= sodium sulfate decahydrate, Na2SO4⋅10H2O The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. 1.) Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 1.00? mass= 2.)Based on this information, what volume of acid should the student measure to make the buffer solution? volume=
To fill a 500 mL volumetric flask, 40 g of ammonium chloride (NH4Cl) and 3.2 g of ammonia (NH3) are added along with water. Given the Kb of NH3 is 1.8 × 10−5, the pH of this buffer is...