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In a food and drink industry, sulphur dioxide is often used as a preservative. By gravimetric analysis, the content of sulphur dioxide in dried peaches was calculated as follows: The dried peaches were powdered in a blender. A sample of the peach powder weighing 45.0692 g was put into a conical flask containing 100 mL of deionized water. A 3% solution of hydrogen peroxide was added to convert the dissolved sulphur dioxide to sulphate ions. The conversion of sulphur dioxide to sulphuric acid is shown in the half equation: SO2 (aq) + 2H2O (I) O SO,? (aq) + 4H* (aq) + 2e- An excess of calcium chloride solution was then added. The calcium sulphate precipitate was filtered off, dried and weighed to constant mass. The equation for the precipitation of calcium sulphate is Ca?*(aq) + SO, (aq) => CaSO4(s) The following results were recorded. i. ii. ii. iv. V. Mass of dry filter paper 0.951 g Mass of dry filter paper and CaSO4 sample 1.538 g Determine the percentage, by mass, of SO2 in the peach sample.

In a food and drink industry, sulphur dioxide is often used as a preservative. By gravimetric analysis, the content of sulphur dioxide in dried peaches was calculated as follows: The dried peaches were powdered in a blender. A sample of the peach powder weighing 45.0692 g was put into a conical flask containing 100 mL of deionized water. A 3% solution of hydrogen peroxide was added to convert the dissolved sulphur dioxide to sulphate ions. The conversion of sulphur dioxide to sulphuric acid is shown in the half equation: SO2 (aq) + 2H2O (I) O SO,? (aq) + 4H* (aq) + 2e- An excess of calcium chloride solution was then added. The calcium sulphate precipitate was filtered off, dried and weighed to constant mass. The equation for the precipitation of calcium sulphate is Ca?*(aq) + SO, (aq) => CaSO4(s) The following results were recorded. i. ii. ii. iv. V. Mass of dry filter paper 0.951 g Mass of dry filter paper and CaSO4 sample 1.538 g Determine the percentage, by mass, of SO2 in the peach sample.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
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b) In a food and drink industry, sulphur dioxide is often used as a preservative. By gravimetric analysis, the content of sulphur dioxide in dried peaches was calculated as follows: i. The dried peaches were powdered in a blender. A sample of the peach powder weighing 45.0692 g was put into a conical flask containing 100 mL of deionized water. ii. iii. A 3% solution of hydrogen peroxide was added to convert the dissolved sulphur dioxide to sulphate ions. The conversion of sulphur dioxide to sulphuric acid is shown in the half equation: SO2 (aq) + 2H2O (I) O SO,? (aq) + 4H* (aq) + 2e- An excess of calcium chloride solution was then added. The calcium sulphate precipitate was filtered off, dried and weighed to constant mass. The equation for the precipitation of calcium sulphate is Ca?+(aq) + SO? (aq) => CaSO:(s) The following results were recorded. iv. V. Mass of dry filter paper 0.951 g Mass of dry filter paper and CaSO4 sample 1.538 g Determine the percentage, by mass, of SO2 in the peach sample.
Transcribed Image Text:b) In a food and drink industry, sulphur dioxide is often used as a preservative. By gravimetric analysis, the content of sulphur dioxide in dried peaches was calculated as follows: i. The dried peaches were powdered in a blender. A sample of the peach powder weighing 45.0692 g was put into a conical flask containing 100 mL of deionized water. ii. iii. A 3% solution of hydrogen peroxide was added to convert the dissolved sulphur dioxide to sulphate ions. The conversion of sulphur dioxide to sulphuric acid is shown in the half equation: SO2 (aq) + 2H2O (I) O SO,? (aq) + 4H* (aq) + 2e- An excess of calcium chloride solution was then added. The calcium sulphate precipitate was filtered off, dried and weighed to constant mass. The equation for the precipitation of calcium sulphate is Ca?+(aq) + SO? (aq) => CaSO:(s) The following results were recorded. iv. V. Mass of dry filter paper 0.951 g Mass of dry filter paper and CaSO4 sample 1.538 g Determine the percentage, by mass, of SO2 in the peach sample.
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