diprotic acid. The procedure for identifying an unknown acid is exactly as described in the lab manual. Part 1: Standardization of NaOH. 1.4378 g of oxalic acid was dissolved in 250.0 mL of water and a 25.00 m aliquote was titrated with NaOH. 24.73 mL of titrant was required. Determine the concentration of sodium hydroxide. Answer: Part 2: Titration of the unknown acid. 1.9875 g of the unknown acid was dissolved in 250.0 ml of water and 25.00 ml of this solution was titrated with the NaOH. 29.50 mL of titrant was required. Determine the Molar Mass of the unknown. Answer:

diprotic acid. The procedure for identifying an unknown acid is exactly as described in the lab manual. Part 1: Standardization of NaOH. 1.4378 g of oxalic acid was dissolved in 250.0 mL of water and a 25.00 m aliquote was titrated with NaOH. 24.73 mL of titrant was required. Determine the concentration of sodium hydroxide. Answer: Part 2: Titration of the unknown acid. 1.9875 g of the unknown acid was dissolved in 250.0 ml of water and 25.00 ml of this solution was titrated with the NaOH. 29.50 mL of titrant was required. Determine the Molar Mass of the unknown. Answer:

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 77QAP: Two students were asked to determine the Kb of an unknown base. They were given a bottle with a...

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Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or base? Explain.
Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
. For each hydrogen or hydroxide ion concentration listed. calculate the concentration of the complementary ion and the pH and pOH of the solution. a. [H+]=5.72104M b. [OH-]=8.91105Mc. [H+]=2.871012Md. [OH-]=7.22108M
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.
Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 M
A 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000