Styles2. Use a 100-mL beaker to make a 50 ml of the sodium acetate (NaA)/acetate (HA) buffersolution, as shown in the table. Measure and record the pH. Pipette 25 ml of this buffersolution and place it in a new 50-ml beaker. Add 1 ml of 1 M HCI or 1 M NAOH to eachseparate beaker and mix well. Measure and record pH.Table 2:Buffered solution (acetate)Calculated pHMeasuredpH25 mL 1.0 M NaAc + 25 ml 1.0M HA4.234.1225 ml above mix buffer +1 ml 1.0 M HCI4.2225 ml above mix buffer + 1 ml 1.0 M NAOHD, Focus* The pka of acetic acid is 4.75.

pH of the buffer can be calculated using Hasselbach-Henderson equation pH =pKa +log [NaA][HA]

Answered: Styles 2. Use a 100-mL beaker to make a…

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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Consider a 1.0 L buffer containing 0.095 mol L-1 HCOOH and 0.1 mol L-1 HCOO-. What is the pH of the solution after adding 1.6 x 10-3 mol of NaOH? Express your answer to 2 decimal places. Remember you can find KA and/or KB values in your textbook in chapter 15. They are also posted on eClass.
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…
Calculate H+ and pka (given is pH) refer to the picture below. Please include your solution. PLEASE ANSWER QUESTIONS 1-3 and use the 2nd picture for the formula that must be used
Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH
show calculations for how the pH of each of these solutions would be determined. a. Buffer solution prepared from 10.00 mL of 1.0 M HC2H3O2 and 10.00 mL of 1.0 M NaC2H3O2 b. 20.00 mL of buffer solution with 1.00 mL of 1.0 M NaOH. c. 20.00 mL of buffer solution with 1.00 mL of 1.0 M HCl. d. 20.00 mL of water with 1.00 mL of 1.0 M NaOH added e. 20.00 mL of water with 1.00 mL of 1.0 M HCl added
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a) Compare between equivalence point and endpoint. Distinguish which point comes first. b) James performed an acid base titration experiment. A 25 mL sample containing HCl was transferred to Erlenmeyer flask using volumetric pipette. HCl sample was titrated against standardized 0.5010 M NaOH. An average titre volume of 24.35 mL was reported. Suggest a suitable pH indicator for James to be used in this experiment. Predict the initial concentration of the HCl. c) Alan and friends wish to sketch a weak acid strong base titration curve. Before they can do so, they need some data points. In a case where 50 mL of 0.20 M CH3COOH (Ka = 1.80 x 10-5 ) was titrated with 0.05 M NaOH, deduce the pH after addition of different volumes of NaOH. (i) 0 mL NAOH (ii) 100 mL NaOH (iii) 200 mL NaOH
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You are asked to make the 4.5 pH buffer from question the previous question. a. From the list of Acids and conjugate bases attached which pair would you pick. b. You are asked to make a 2M stock solution of the Buffer, how many grams of each acid and base would you need to make a 1000mL stock. c. For the experiment, the final concentration of the buffer should be 50mM. How many mL of your stock would you need to make 2L. Hint: M1V1=M2V2

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