Question

Saccharin, an artificial sweetener, has the formula $\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{S} .$ Suppose you have a sample of a saccharincontaining sweetener with a mass of $0.2140 \mathrm{g}$. After decomposition to free the sulfur and convert it to the $\mathrm{SO}_{4}^{2-}$ ion, the sulfate ion is trapped as water-insoluble BaSO, (Figure 4.6 ). The quantity of BaSO, obtained is $0.2070 \mathrm{g} .$ What is the mass percent of saccharin in the sample of sweetener?

          Saccharin, an artificial sweetener, has the formula $\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{S} .$ Suppose you have a sample of a saccharincontaining sweetener with a mass of $0.2140 \mathrm{g}$. After decomposition to free the sulfur and convert it to the $\mathrm{SO}_{4}^{2-}$ ion, the sulfate ion is trapped as water-insoluble BaSO, (Figure 4.6 ). The quantity of BaSO, obtained is $0.2070 \mathrm{g} .$ What is the mass percent of saccharin in the sample of sweetener?

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Added by Remedios C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Madhur L

08/22/2023

Step 1

First, we need to find the molar mass of saccharin, BaSO4, and SO4^2-. Saccharin: C7H5NO3S Molar mass of saccharin = (7 × 12.01) + (5 × 1.01) + 14.01 + (3 × 16.00) + 32.07 = 183.18 g/mol BaSO4: Molar mass of BaSO4 = 137.33 + 32.07 + (4 × 16.00) = 233.43 Show more…

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Saccharin, an artificial sweetener, has the formula $mathrm{C}_{7} mathrm{H}_{5} mathrm{NO}_{3} mathrm{S} .$ Suppose you have a sample of a saccharincontaining sweetener with a mass of $0.2140 mathrm{g}$. After decomposition to free the sulfur and convert it to the $mathrm{SO}_{4}^{2-}$ ion, the sulfate ion is trapped as water-insoluble BaSO. The quantity of BaSO obtained is $0.2070 mathrm{g} .$ What is the mass percent of saccharin in the sample of sweetener?

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