Styles 2. Use a 100-mL beaker to make a 50 ml of the sodium acetate (NaA)/acetate (HA) buffer solution, as shown in the table. Measure and record the pH, Pipette 25 ml of this buffer solution and place it in a new 50-ml beaker. Add 1 ml of 1 M HCI or 1 M NaOH to each separate beaker and mix well. Measure and record pH. Table 2: Buffered solution (acetate) Calculated pH

Styles 2. Use a 100-mL beaker to make a 50 ml of the sodium acetate (NaA)/acetate (HA) buffer solution, as shown in the table. Measure and record the pH, Pipette 25 ml of this buffer solution and place it in a new 50-ml beaker. Add 1 ml of 1 M HCI or 1 M NaOH to each separate beaker and mix well. Measure and record pH. Table 2: Buffered solution (acetate) Calculated pH

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.43QE: A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the...

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The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
A buffer solution that is 0.100 M acetate ion and 0.100 M acetic acid is prepared. (a) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL of the buffer. (b) Calculate the initial pH, final pH, and change in pH when 1.00 mL of 1.00 M NaOH is added to 100.0 mL pure (pH 7.00) water.
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)?
4. Use a 100-mL beaker to make 50 ml of sodium phosphate solution by mixing 0.8 ml of 2 M monobasic NaH;PO4, 4.2 ml of 2 M dibasic N2>HPO4, and 45 ml of H20 as shown in the table. Measure and record the pH. Pipette 20mL of this buffer solution and place it in a new 50-ml beaker. Add 1 ml of 1 M HCI or 1 M NaOH to each separate beaker and mix well. Measure and record the pH. Table 4: Buffered solution (phosphate) Calculated pH Measured pH 0.8 mL of 2 M monobasic NaH,PO4 + 4.2 mL 7.66 of 2 M dibasic Na>HPO4 + 45 mL H20 25 ml above mix buffer +1 ml 1.0 M HCI 7.08 25 ml above mix buffer +1 mL 1.0 M NaOH 7.71 * The pKaz and pkaz of phosphate groups are 6.8 and 12.3, respectively.
Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO and combine them into a beaker. This is the buffer solution Measure out 50.0 mL of the buffer in part D (that you just made) and pour it into a clean beakerand add 2.0 mL of 1.0 M NaOH to it. What is the calculated/expected pH of this solution after the addition of the NaOH?
Measure out 50.0 mL 1.0 M CH3COOH and 50.0 mL of 1.0 M NaCH3COO and combine them into a beaker. This is the buffer solution Measure out 50.0 mL of the buffer in part D (that you just made) and pour it into a clean beakerand add 2.0 mL of 1.0 M HCl to it. What is the calculated/expected pH of this solution after the addition of the HCl?
A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH. A) Calculate the pH at 0 mL of added base. Express your answer using two decimal places. B)Calculate the pH at 5 mL of added base. Express your answer using two decimal places. C) Calculate the pH at 10 mL of added base. Express your answer using two decimal places. D) Calculate the pH at the equivalence point. Express your answer using two decimal places. E)Calculate the pH at one-half of the equivalence point. Express your answer using two decimal places. F) Calculate the pH at 20 mL of added base. Express your answer using two decimal places. G) Calculate the pH at 25 mL of added base. Express your answer using two decimal places.
4. A 100 mL buffer solution with pH of 4.80 is prepared as a stock solution. Using this stock buffer solution, three buffers are prepared by diluting a given volume of the stock buffer (as shown below) to 100 mL with water. Buffer 1 a. b. e a. E Do they have the same pH? Check the box corresponding your answer. Yes No Which is true about their absolute concentrations? Check the box corresponding your answer. [Buffer 1]> [Buffer 2] > [Buffer 3) [Buffer 3] > [Buffer 2]> [Buffer 1] [Buffer 3] = [Buffer 2] = [Buffer 1) [Buffer 3] = [Buffer 2] > [Buffer 1) [Buffer 3] > [Buffer 2] = [Buffer 1) d. Which of the following is true about the ability of the three buffers to resist pH change when 1 mL of HCI is added to each buffer? Check the box corresponding your answer. Which is true about their concentration ratios? Check the box corresponding your answer. [Buffer 1]> [Buffer 2] > [Buffer 3) [Buffer 3] > [Buffer 2]> [Buffer 1) [Buffer 3] = [Buffer 2] = [Buffer 1) Solution A B C D [Buffer 3] =…
1. A student titrates 25.0 mL of an unknown base with 0.10 M HCI. During the titration the pH is monitored and the collected data is recorded. These data are shown in the table at the right. a. Use the information provided to draw a titration curve showing the pH as a function of the volume of added HCI. Be certain to label your axes. b. Identify the equivalence point on your graph and justify your selection of this particular point. c. Use the data to determine the Kö value for the weak base. Be certain to show the mathematical steps you take to arrive at the answer. Report your final answer to the correct number of significant digits. d. The student has three indicators that she could use for this experiment. The indicators (with their endpoints) are: Bromophenol Blue (3.0 - 4.6), Methyl Red (4.2 – 6.3), and phenolphthalein (8.3 – 10.0). Which indicator would be appropriate for this titration? Justify your selection. e. Determine the (i) molarity and the (ii) % ionization of the…
Now your turn! Sketch the neutralisation curve when 40 cm³ of 0.50 moldm³ sodium hydroxide solution is added to 20.0 cm³ of 0.40 moldm³ propanoic acid (pKa = 4.9). ● Extension: Consider whether methyl orange is an appropriate indicator to find the end point of this titration MacBook Air
Describe/ explain what a buffer is/ how it works. Do Not use the words "acid" or "base" or any derivative of those (e.g. "acidic", "basic", etc.)?