Titrating ascorbic acid with iodine is what type of titration?HO.HO.+ 2 HIHO3x-3x=h+HOHOOHIodineAscorbic AcidDehydro-Ascorbic AcidO An acid-base neutralization titration, because iodine is a strong acidOA redox titration, because iodine acts as an oxidizing agentOA redox titration, because iodine acts as a reducing agentAn acid-base neutralization titration, because ascorbic acid is a weak base

This iodometric reaction is a well-known redox titration method used to determine vitamin C (or…

Answered: Titrating ascorbic acid with iodine is…

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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Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10-⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the solution pH when 10.00 mL of titrant have been added? (Two decimal places) Type your answer...
O ACIDS AND BASES Calculating the pH of a weak acid titrated with a strong base pH An analytical chemist is titrating 240.9 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 0.2500M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 630.6 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. = 0 X 1/5 S Sabrina
When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH = 35.9 mL sample of a 0.576 M aqueous hypochlorous acid solution is titrated with a 0.329 M aqueous sodium hydroxide solution. What is the pH after 42.9 mL of base have been added? Ka for HC1O is 3.5 × 10-8. pH = A 26.3 mL sample of 0.296 M ethylamine, C₂H5NH₂, is titrated with 0.246 M perchloric acid. At the titration midpoint, the pH is A 20.0 mL sample of 0.369 M diethylamine, (C₂H5)₂NH, is titrated with 0.320 M perchloric acid. After adding 8.88 mL of perchloric acid, the pH is
Which of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M sodium nitrite 0.31 M ammonium bromide + 0.31 M ammonia 0.29 M hydroiodic acid + 0.23 M potassium iodide 0.16 M potassium fluoride + 0.21 M hydrofluoric acid O 0.39 M acetic acid + 0.25 M potassium acetate
Which of the following aqueous solutions are good buffer systems? O0.13 M hypochlorous acid + 0.12 M sodium hypochlorite O 0.10 M potassium fluoride + 0.30 M hydrofluoric acid 0.27 M hydrobromic acid + 0.23 M potassium bromide 0.39 M acetic acid + 0.28 M potassium acetate O 0.34 M ammonium nitrate + 0.38 M ammonia
3 A student performs a titration of 53.0 mL of a phosphoric acid (H₂PO) solution of unknown concentration with a standardized 1.25 M NaOH solution. The titration requires 26.2 mL of base to reach the third equivalence point. What is the concentration of the H,PO solution? 3
700. ml of HBr solution of unknown concentration is titrated to the equivalence point using 730. ml of 0.90 M NaOH solution. What was the concentration of the HBr solution? O 11M O 13M O 0.76 M O 0.94 M
7B-3. A 15.00 mL sample of an unknown perchloric acid solution is titrated with a 0.687 M barium hydroxide solution. It takes 29.31 mL of the base solution to reach the endpoint. а. Write a balanced chemical equation for the reaction that occurs. b. What is the molarity of the unknown acid solution?
What is one of the products formed when potassium hydroxide and hydrochloric acid are used in titration? hydrogen gas free oxygen water O potassium oxide What are needed to form an ammonium hydroxide solution?* O NO2 and H20 N2 and H20 O NH3 and H20 O NO2 and dilute NaOH
Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI
Which of the following aqueous solutions are good buffer systems? 0.18 M barium hydroxide + 0.22 M barium bromide O0.11 M acetic acid + 0.19 M hydrobromic acid 0.33 M sodium perchlorate + 0.25 M calcium perchlorate O 0.28 M hydrochloric acid + 0.20 M sodium chloride 0.30 M ammonia + 0.37 M ammonium bromide
Which of the following aqueous solutions are good buffer systems? O 0.36 M hydrofluoric acid + 0.23 M potassium fluoride O 0.27 M hydrochloric acid + 0.22 M sodium chloride O 0.15 M potassium hydroxide + 0.24 M potassium chloride O 0.15 M hydrocyanic acid + 0.15 M sodium cyanide O 0.27 M ammonium bromide + 0.33 M ammonia

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