56. What is the number of moles of HCI contained in the 12-mL solution added? 57. What is the number of moles of CH3COOH which participated in the reaction upon adding 12 mL of 1.5 M HCI? 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?

56. What is the number of moles of HCI contained in the 12-mL solution added? 57. What is the number of moles of CH3COOH which participated in the reaction upon adding 12 mL of 1.5 M HCI? 58. What is the number of moles of CH3COOK which participated in the reaction upon adding 12 mL of 1.5 M HCI? 59. What is the pH of the original buffer solution? 60. What is the pH of the final buffer solution? 61. What is the final ratio of the CH3COOH and CH3COOK? 62. What is the change in pH in percentage?

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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Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (p?a=4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH= What volume of 2.50 M NaOH would be required to increase the pH to 4.93? volume:
1. The number of moles of HCl contained in the 12-mL solution added 2. The number of moles of CH3COOH which participated in the reaction upon adding 12-mL of 1.5 M HCl 3. The number of moles of CH3COOK which participated in the reaction upon adding 12-mL of 1.5 M HCl 4. The pH of the original buffer solution 5. The pH of the final buffer solution 6. The final ratio of the CH3COOH and CH3COOK 7. The change in pH, in percentage *Use 2 decimal places
5. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4 a. What is the pH of this buffer? b. If 0.075 mol HCI is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes) c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)
A buffer solution contains 0.240 M CH,NH,Br and 0.455 M CH,NH, (methylamine). Determine the pH change when 0.107 mol HI is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change
Use the Henderson–Hasselbalch equation to calculate the pH of each solution.a. a solution that is 0.135 M in HClO and 0.155 M in KClOb. a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH3Br by massc. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution
A 200. mL sample of buffer contains 1.20 M CH3NH2 (methylamine) and 1.00 M CH3NH3Cl (methylammonium chloride). a. Write the net ionic equation that shows how the buffer will react with added generic acid H+. b. Write the net ionic equation that shows how the buffer will react with added generic base OH–. c. Determine the pH of this buffer solution. d. Determine the pH of this solution after the addition of 8.0 mL 5.0 M HBr. e. Phenol red is an organic compound that can be used as an acid/base indicator with pKa = 7.2. The two different forms and colors of phenol red are shown. At the pH you determined in part b, what color would you expect the phenol red indicator to be? (Circle one.) yellow, orange, pink, cannot predict
A buffer is created by adding 0.125 moles of hypobromous acid (HOBr, pKa = 8.65) and 0.475 moles of sodium hypobromite (NaOBr) to 1.00 L of solution.25.00 mL of 0.200 M HCl is then added to the solution.a) What is the pH of the solution after the acid is added?
A buffer pair consists of a conjugate weak acid0weak base pair that will resist a change in pH from the addition of a strong acid or base. Decide whether each pair below is a good example of a buffer.a. HCN and NaCN Good Buffer or Not a Bufferb. H2CO3 and Na2CO3 Good Buffer or Not a Bufferc. H2SO4 and NaHSO4 Good Buffer or Not a Buffer
22. Which of the following mixture could be considered as a buffer? Hint: Try to react each mixture (if possible) and look for a pair that could be components for the buffer c. HC1 + CF d. CH3COO+ OH- a. NH4C1 + NAOH b. NH3 + NaOH 23. What is the pH of a buffer solution containing 0.25 M acetic acid and 0.030 M sodium acetate? The acid dissociation constant for acetic acid is equal to 1.8 x 10 Hint no dilution occurred a. 3.82 b. 5.67 C. 10.18 d. 8.34
A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. What is the concentration (M) of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCI to 25.0 mL of this solution? Select one: Oa. 0.130 Ob. 0.122 OC. 0.0953 Od. 0.0900
Consider the titration curve for a diprotic acid: 12 10 8 pH 6 4+ 2 + + 10 20 30 Volume of NaOH added (mL) Label the curve with the following items: first equivalence point, second equivalence point, first halfway point, halfway between first and second equivalence points. Determine K, and K, for this diprotic acid. al a2
2. A buffer solution contains 0.15 mol of propionic acid (HC3H5O2) and 0.10 mol of sodium propionate (NaC3H5O2) in 1.20 L of the solution. What is the pH of the buffer after the addition of 0.01 mol of NaOH?