A 4.85 cm3 fruit juice sample was titrated against 7.5 x 10-4 mol/L iodine solution, using starch indicator. The average titre was 21.23 cm3. Given the molecular mass of Vitamin C (C6H8O6) is 176 g/mol, and the redox equation: C6H8O6(aq) + I2(aq)→C6H6O6(aq) + 2H+(aq) + 2I-(aq) Calculate the mass of Vitamin C per mL of fruit juice.

A 4.85 cm3 fruit juice sample was titrated against 7.5 x 10-4 mol/L iodine solution, using starch indicator. The average titre was 21.23 cm3. Given the molecular mass of Vitamin C (C6H8O6) is 176 g/mol, and the redox equation: C6H8O6(aq) + I2(aq)→C6H6O6(aq) + 2H+(aq) + 2I-(aq) Calculate the mass of Vitamin C per mL of fruit juice.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.103QE

See similar textbooks

Similar questions

A sample of CaCO3 (molar mass=100.1) weighing 0.4856 g is dissolved in HCl and the solution diluted to 500.0 mL in a volumetric flask. A 25.00-mL aliquot requires 21.37 mL of an EDTA solution for titration. How many grams of Na2H2Y.2H2O (molar mass=372.2) are required to prepare 500.0 mL of this solution.
Titration of 0.1756 grams primary standard sodium oxalate (134.00 g/mol) dissolved in 50 mL water with 5 mL concentrated sulfuric acid required 32.1 mL of a potassium permanganate solution. redox method used?Which served as the oxidizing agent? Which served as the reducing agent?What is the total number of electrons involved in the redox reaction?What can be used as an indicator for the titration?What is the molar concentration of the titrant?
The amount of ascorbic acid, C6H8O6, in orange juice was determined by oxidizing the ascorbic acid to dehydroascorbic acid, C6H6O6, with a known excess of I3–, and back titrating the excess I3– with Na2S2O3. A 5.00-mL sample of filtered orange juice was treated with 50.00 mL of excess 0.01003 M I3–. After the oxidation was complete, 12.2722 mL of 0.06729 M Na2S2O3 was needed to reach the starch indicator end point. Report the concentration of ascorbic acid in milligrams per 100 mL.
A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?
Titration of 0.1756 grams primary standard sodium oxalate (134.00 g/mol) dissolved in 50 mL water with 5 mL concentrated sulfuric acid required 32.1 mL of a potassium permanganate solution. Which served as the reducing and oxidizing agent? What can be used as an indicator for thetitration? What is the molar concentration of the titrant? What is the total number of electrons involved in the redox reaction? What type of redox method was used?
If the copper standard solution has a concentration of 25 μg/mL, what is the concentration of a prepared solution with 4 mL of the standard solution with 2 mL 10% hydroxylamine hydrochloride, 5 mL 10% ammonium acetate, and 5 mL of 0.1% bathocuproine prepared in a 25 mL volumetric flask?
A 11.00 gram sample of Vodka was analysed for its alcohol content. The sample was placed in a300 mL volumetric flask and made to the mark with distilled water. A 20.0 mL aliquot of the dilutedVodka was taken from the volumetric flask and placed in a conical flask containing some distilled water from a previous washing.The 20.0 mL aliquots were titrated against a 0.1302 M Cr2O72-solution and an average titre of13.25 mL was obtained.The reaction between the alcohol and the dichromate solution is given below2Cr2O72–(aq) + 3CH3CH2OH(aq) + 16H+(aq)  4Cr3+(aq) + 3CH3COOH(aq) + 11H2O(l)a) Calculate the amount in mol of Cr2O72– in the average titre. b) Calculate the percentage, by mass, of ethanol in the vodka.
A solution of citric acid (H₃C₆H₅O₇) with a known concentration of 0.200 M H₃C₆H₅O₇ is titrated with a 0.750 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 25.0 mL H₃C₆H₅O₇ , according to the following balanced chemical equation: H₃C₆H₅O₇ + 3 NaOH → Na₃C₆H₅O₇ + 3 H₂O
A 10.0-mL sample of sulfuric acid, H2SO4, from a battery of an old car is diluted to 100.0 mL, and a 10.00-mL aliquot (portion) of the diluted acid is then titrated with 0.2500 M NaOH solution. If the concentration of H2SO4 in the original battery was 3.25 M, how many milliliters (mL) of the NaOH solution is required to titrate the sulfuric acid present in the 10.0-mL portion of dilute acid solution? This acid-base reaction occurs as follows:
A 10.0-mL sample of sulfuric acid, H2SO4, from a battery of an old car is diluted to 100.0 mL, and a 10.00-mL aliquot (portion) of the diluted acid is then titrated with 0.2500 M NaOH solution. If the concentration of H2SO4 in the original battery was 3.25 M, how many milliliters (mL) of the NaOH solution is required to titrate the sulfuric acid present in the 10.0-mL portion of dilute acid solution? This acid-base reaction occurs as follows: H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(g) (A) 130. mL (B) 65.0 mL (C) 26.0 mL (D) 13.0 mL
Concentration of NaOCl in Full-strength Commercial Bleach: A diluted bleach solution was found to have a concentration of 0.0284 M. It was originally prepared by diluting 3.0 mL of full-strength commercial bleach, with water, to a total volume of 100.00 mL. What is the molar concentration of NaOCl in the full-strength commercial bleach solution?
A solution is prepared by pipetting 25.0 mL of 0.350 M CuCl2 into a 100.0 mL volumetric flask, diluting to the calibration mark on the flask with water and quantitatively mixing the contents of the flask. What is the molar concentration of Cl- in the solution?