Trial 25.58mL Volume of NaOH added to reach the equivalence point : Volume of NaOH added to reach the 1/2 equivalence point: 12.79mL 4.45 PH @ 1/₂ the equivalence point: pha of unknown acid: ≈ 4.45 Average pha of unknown Acid: 4.6 Possible Identity of unknown weak acid: Molarity of unknown acid: Trial 2 25.32mL 12.66mL 4.75 ~4.75

Trial 25.58mL Volume of NaOH added to reach the equivalence point : Volume of NaOH added to reach the 1/2 equivalence point: 12.79mL 4.45 PH @ 1/₂ the equivalence point: pha of unknown acid: ≈ 4.45 Average pha of unknown Acid: 4.6 Possible Identity of unknown weak acid: Molarity of unknown acid: Trial 2 25.32mL 12.66mL 4.75 ~4.75

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 1P

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A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
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.
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
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