Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 106

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 \(0.0522~g\), and the average mass percent of saccharin in the tablets is \(88.56\%\).

Step by step solution

01

Calculate the moles of BaSO4 obtained

First, we need to find the moles of BaSO4 obtained from the given mass. The molar mass of BaSO4 is: \(M_{BaSO_4} = (137.33 + 32.07 + (4 × 16))~g/mol\) Moles of BaSO4 can be calculated as: \(moles~BaSO4 = \frac{mass~BaSO4}{M_{BaSO4}}\)
02

Find the moles of sulfur present in the saccharin tablets

Since all the sulfur in saccharin is converted to sulfate ions in the obtained BaSO4, we can determine the moles of sulfur present in the saccharin tablets. \(moles~S = moles~BaSO4\)
03

Determine the mass of saccharin and calculate its average mass per tablet

Now that we have the moles of sulfur, we can calculate the mass of saccharin (C7H5NO3S). The molar mass of saccharin is: \(M_{saccharin} = (7 × 12.01 + 5 × 1.01 + 1 × 14.01 + 3 × 16 + 1 × 32.07)~g/mol\) Mass of saccharin can be found by: \(mass~saccharin = moles~S × M_{saccharin}\) Then we can find the average mass of saccharin per tablet as: \(average~mass~per~tablet = \frac{mass~saccharin}{10}\)
04

Calculate the average mass percent of saccharin in the tablets

Finally, we can calculate the average mass-percent of saccharin in the tablets using the formula: \(mass~percent = \frac{average~mass~saccharin~per~tablet}{average~mass~per~tablet} × 100\) Where "average mass per tablet" refers to the total mass of the tablets divided by 10.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Using the general solubility rules given in Table 4.1, name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions. a. chloride ion b. calcium ion c. iron(III) ion d. sulfate ion e. mercury(I) ion, \(\mathrm{Hg}_{2}{ }^{2+}\) f. silver ion

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{KMnO}_{4}\) b. \(\mathrm{NiO}_{2}\) c. \(\mathrm{Na}_{4} \mathrm{Fe}(\mathrm{OH})_{6}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) e. \(\mathrm{P}_{4} \mathrm{O}_{6}\) f. \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) g. \(\mathrm{XeOF}_{4}\) h. \(\mathrm{SF}_{4}\) i. CO j. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) b. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{KOH}(a q) \rightarrow\) c. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Which of the following solutions of strong electrolytes contains the largest number of moles of chloride ions: \(100.0 \mathrm{~mL}\) of \(0.30 \mathrm{M} \mathrm{AlCl}_{3}, 50.0 \mathrm{~mL}\) of \(0.60 \mathrm{M} \mathrm{MgCl}_{2}\), or \(200.0 \mathrm{~mL}\) of \(0.40 \mathrm{M} \mathrm{NaCl} ?\)

What volume of each of the following bases will react completely with \(25.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\) ? a. \(0.100 \mathrm{M} \mathrm{NaOH}\) b. \(0.0500 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\) c. \(0.250 \mathrm{M} \mathrm{KOH}\)
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free