A group of chemistry students determined the titratable acidity of two brands of tetrapack juice. Titratable acidity is a measure of the total acid concentration in a food sample. Titratable acidity in fruit juices is commonly expressed in terms of milligrams (mg) of hydrous citric acid (H3CitH20, MM: 210.14 g/mol) per mL solution. Initially, they have prepared the sodium hydroxide solution and standardized it with oxalic acid dihydrate (H2C204-2H20; MM:126.02 g/mol; 99.5% purity) up to the faint pink endpoint of phenolphthalein. The volumes of the duplicate trial of the standardization were summarized in the table. In the sample analysis, 5.00mL each of tetra pack juice was diluted with 50.0 mL of distilled water and titrated up to an endpoint of 8.2 using a pH meter. Consider the tables below and answer the following questions. Table 1. Standardization of the NaOH titrant grams of primary standard Volume NaOH used (mL) 0.2490 39.4 0.2510 39.5 Table 2. Titration of the samples with the standardized titrant. Volume Readout of Burette (mL, NAOH) Sample Initial Final Brand X 0.00 1.90 Brand Y 2.10 3.60 What is the molarity of the titrant? M Note: it requires 3 moles of hydroxide to titrate 1 mole of citric acid Calculate the molarity of citric acid in both of the samples? Band X sample. Brand Y sample M

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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Transcribed Image Text:A group of chemistry students determined the titratable acidity of two brands of tetrapack juice. Titratable acidity is a measure of the total acid concentration in a food sample. Titratable acidity in fruit juices is commonly expressed in terms of milligrams (mg) of hydrous citric acid (H3CitH20, MM: 210.14 g/mol) per mL solution. Initially, they have prepared the sodium hydroxide solution and standardized it with oxalic acid dihydrate (H2C204 2H20; MM:126.02 g/mol; 99.5% purity) up to the faint pink endpoint of phenolphthalein. The volumes of the duplicate trial of the standardization were summarized in the table. In the sample analysis, 5.00ML each of tetra pack juice was diluted with 50.0 mL of distilled water and titrated up to an endpoint of 8.2 using a pH meter. Consider the tables below and answer the following questions. Table 1. Standardization of the NaOH titrant grams of primary standard Volume NaOH used (mL) 0.2490 39.4 0.2510 39.5 Table 2. Titration of the samples with the standardized titrant. Volume Readout of Burette (mL, NaOH) Sample Initial Final Brand X 0.00 1.90 Brand Y 2.10 3.60 What is the molarity of the titrant? M Note: it requires 3 moles of hydroxide to titrate 1 mole of citric acid Calculate the molarity of citric acid in both of the samples? Band X sample. Brand Y sample M

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