A student is asked to determine the value of Ka for hypochlorous acid by titration with barium hydroxide. The student begins titrating a 41.7 mL sample of a 0.453 M aqueous solution of hypochlorous acid with a 0.375 M aqueous barium hydroxide solution, but runs out of standardized base before reaching the equivalence point. The student's last observation is that when 16.3 milliliters of barium hydroxide have been added, the pH is 7.763. What is Ka for hypochlorous acid based on the student's data?

A student is asked to determine the value of Ka for hypochlorous acid by titration with barium hydroxide. The student begins titrating a 41.7 mL sample of a 0.453 M aqueous solution of hypochlorous acid with a 0.375 M aqueous barium hydroxide solution, but runs out of standardized base before reaching the equivalence point. The student's last observation is that when 16.3 milliliters of barium hydroxide have been added, the pH is 7.763. What is Ka for hypochlorous acid based on the student's data?

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...

See similar textbooks

Similar questions

You set up a titration in the lab to determine the concentration of an HCl solution. What is the molarity of an HCl solution if 0.0100 L of 0.245 M NaOH soln’ are required to neutralize 0.0150 L HCl? 2.25 M 0.163 M 1.34 M 0.245 M
Acetic Acid Titration with NaOH. 50.00 ml of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to reach the endpoint of the titration. What is the molarity of the acetic acid solution? (Do NOT include units)
A 35.8 mL sample of a 0.321 M aqueous acetic acid solution is titrated with a 0.408 M aqueous potassium hydroxide solution. What is the pH after 17.3 mL of base have been added?
I have a 50.0 mL sample of a solution of hydrocyanic acid, HCN, of unknown concentration. I titrate the HCN solution with a stock solution of 10.0 M NaOH. I reach endpoint when 6.50 mL of LIOH solution have been added. What is the original concentration of my HCN solution?
A 21.3 mL sample of a 0.387 M aqueous nitrous acid solution is titrated with a 0.333 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added? pH =
Please help me find the initial concentration of acid (M). This is a titration. Volume of acid (mL): 10.0 Volume of NaOH at equivalence point (mL): 30.1 Milimoles of NaOH to neutralize the acid: 50.0 Milimoles of acid: 50.0 Also could you help me find the average initial concentration?
A student conducting this experiment measures out 0.913 g of an unknown monoprotic weak acid and dissolves it in 110 mL of water. After adding an indicator, the student titrates the weak acid with 15.55 mL of 0.380 M NaOH to reach the equivalence point. What is the molar mass of the unknown acid?
A 31.5 mL sample of a 0.489 M aqueous nitrous acid solution is titrated with a 0.425 M aqueous solution of barium hydroxide. How many milliliters of barium hydroxide must be added to reach a pH of 3.158? mL
Suppose 0.442 grams of a solid monoprotic acid are titrated with 15.54 mL of 0.098 M NaOH. What is the molar molar mass of the solid acid?
A student wants to determine the unknown concentration of a sample of sulfuric acid. She performs a titration between her sample of sulfuric acid and potassium hydroxide and collects the data below. Determine the unknown concentration of sulfuric acid.
A 50.0 mL sample of aqueous sodium hydroxide is titrated with 0.425 M sulfuric acid, and 57 mL are required to reach the equivalence point. Write the balanced chemical equation for this reaction. Answer: A 50.0 mL sample of aqueous sodium hydroxide is titrated with 0.425 M sulfuric acid, and 57 mL are required to reach the equivalence point. What is the molarity of the initial sodium hydroxide solution? Hint: You will need the balanced chemical equation you provided as your answer to the previous question. Report your answer to the correct number of significant figures and with the correct units. Answer:
4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100