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Chapter 4: Problem 94

Saccharin \(\left(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S}\right)\) is sometimes dispensed in tablet form. Ten tablets with a total mass of \(0.5894 \mathrm{~g}\) were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of \(\mathrm{BaSO}_{4}\) obtained was \(0.5032 \mathrm{~g}\). What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?

Short Answer

Expert verified
The average mass of saccharin per tablet is \(0.0395 \: g\), and the average mass percent of saccharin in the tablets is \(67.0\% \).

Step by step solution

01

Write the balanced chemical equation for the oxidation of saccharin and precipitation of sulfate

The balanced chemical equation for the oxidation of saccharin (C7H5NO3S) and precipitation of sulfate (BaSO4) is: C7H5NO3S + 4O + BaCl2 -> BaSO4 + 7CO2 + 5H2O + N2 + 2HCl
02

Calculate the moles of BaSO4 formed

Given the mass of BaSO4 obtained, we can calculate the moles of BaSO4. The molar mass of BaSO4 is: \(M_{BaSO4} = 137.3 + 32.1 + (4 × 16.0) = 233.4 \: g/mol\) Now, calculate the number of moles: \(\text{moles of BaSO4} = \frac{\text{mass of BaSO4}}{M_{BaSO4}} = \frac{0.5032 \, g} {233.4 \, g/mol} = 2.156×10^{-3} \:mol \)
03

Calculate the moles of saccharin (C7H5NO3S) in the tablet sample

From the balanced chemical equation, 1 mole of C7H5NO3S produces 1 mole of BaSO4 So, the moles of C7H5NO3S are equal to the moles of BaSO4 formed: \(\text{moles of C}_{7}\text{H}_{5}\text{NO}_{3}\text{S} = 2.156×10^{-3} \: mol\)
04

Calculate the mass of saccharin (C7H5NO3S) in the tablet sample

The molar mass of C7H5NO3S is: \( M_{C7H5NO3S} = (7 × 12.0) + (5 × 1.0) + 14.0 + (3 × 16.0) + 32.1 = 183.2 \: g/mol \) Now, we can find the mass of saccharin: \(\text{mass of C}_{7}\text{H}_{5}\text{NO}_{3}\text{S} = \text{moles} × \text{molar mass} = 2.156×10^{-3} \: \text{mol} × 183.2 \: \text{g/mol} = 0.395 \: g \)
05

Calculate the average mass of saccharin per tablet

To find the average mass of saccharin per tablet, divide the total mass of saccharin by the number of tablets: \(\text{average mass of saccharin per tablet} = \frac{\text{total mass of saccharin}}{\text{number of tablets}} = \frac{0.395 \: g}{10} = 0.0395 \: g \)
06

Calculate the average mass percent of saccharin in the tablets

To find the average mass percent of saccharin in the tablets, divide the mass of saccharin by the total mass of the tablets and multiply by 100: \(\text{average mass \% of saccharin in the tablets} = \frac{\text{total mass of saccharin}}{\text{total mass of tablets}} × 100 = \frac{0.395 \: g}{0.5894 \: g} × 100 = 67.0 \% \) So, the average mass of saccharin per tablet is 0.0395 g, and the average mass percent of saccharin in the tablets is 67.0%.

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Most popular questions from this chapter

A \(30.0\) -mL sample of an unknown strong base is neutralized after the addition of \(12.0 \mathrm{~mL}\) of a \(0.150 \mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is \(0.0300 M\), give some possible identities for the unknown base.

The drawings below represent aqueous solutions. Solution A is \(2.00 \mathrm{~L}\) of a \(2.00 \mathrm{M}\) aqueous solution of copper(II) nitrate. Solution \(\mathrm{B}\) is \(2.00 \mathrm{~L}\) of a \(3.00 \mathrm{M}\) aqueous solution of potassium hydroxide. a. Draw a picture of the solution made by mixing solutions \(\mathrm{A}\) and \(\mathrm{B}\) together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions \(\mathrm{A}\) and \(\mathrm{B}\), and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in \(M\) ) of all ions left in solution (from part a) and the mass of solid formed.

Acetylsalicylic acid is the active ingredient in aspirin. It took \(35.17 \mathrm{~mL}\) of \(0.5065 \mathrm{M}\) sodium hydroxide to react completely with \(3.210 \mathrm{~g}\) of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

Calculate the sodium ion concentration when \(70.0 \mathrm{~mL}\) of \(3.0 \mathrm{M}\) sodium carbonate is added to \(30.0 \mathrm{~mL}\) of \(1.0 \mathrm{M}\) sodium bicarbonate.

In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing \(10.0,25.0,50.0,75.0\), and \(100 .\) ppm of copper from a commercially produced \(1000.0\) -ppm solution? Assume each solution has a final volume of \(100.0 \mathrm{~mL}\). (See Exercise 113 for definitions.)
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