Chemistry III. Calculate the concentration of acetic acid if 20ml of 0.3M was diluted to 100ml withdistilled water.VI. Calculate the Ka of a weak acid if 0.1M solution of the acid gives a PH value of 3.2.VII. Calculate the buffer capacity of each of the following buffers and identify the bestbuffer.Buffer ratioPHPH after addition of 2ml of 0.1M NaOH0.13.703.900.34.24.30.75.25.25

1. M1V1 = M2V2Here , M1 = 0.3MV1 = 20ml , V2 = 100mlM2 = M1V1 / V2 0.3 * 20/ 1OO = 0.06M 2.…

Answered: III. Calculate the concentration of…

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 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

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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.
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)?
Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
3. Calculate the pH of a mixture of 0.25M acetic acid and 0.1 M sodium acetate. pKa of acetic acid is 4.76. I 4. You are required to prepare 1 liter of 0.1 M acetate buffer solution having a pH of 3.5. Calculate the volume of 0.1 M acetic acid and 0.1 M sodium acetate needed in milliliters. (pK, acetic acid is 4.8)
B? The concentrations of acid and base in buffer B are twice the concentrations of buffer A (buffer B is twice as strong as buffer A). Show that the ratio of the volume of titrant required to raise the pH of each buffer 1 unit (VB/VA) is directly related to the ratio of the buffer strengths (strengthe/strengthA) be Buffer capuaty (defined ar Me auoler of naud ar Hhe nuolet ofaud or have needed to change the uubon hu 1 unuf / hy the pH change and voturme huffer ucd in hbres of
Please don't provide handwritten solution ......
Would you calculate the ionic strength of this buffer? [Na2HPO4]=.024176 [NaH2PO4]=.1
-5 A chemistry graduate student is given 450. mL of a 1.00M propanolc acid (HC,H.CO,) solution. Propanolc acid is a weak acid with K 1.3 x 10. What D. mass of KC,H-CO, should the student dissolve in the HC,H.CO, solution to turn it into a buffer with pH =4.41? You may assume that the volume of the solution doesn't change when the KC,H.CO, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
What mass of NH4Cl (Mw = 53.492 g mol-1) has to be dissolved in 750 mL of 0.25 M NH3 (pKa = 9.26) to prepare a buffer with a pH of 9.72?
8. What mass of sodium benzoate should you add to 150.0mL of a 0.15M benzoic acid solution to obtain a buffer with a pH of 4.25?

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