Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 110

A mixture contains only \(\mathrm{NaCl}\) and \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) . A \(1.45-\mathrm{g}\) sample of the mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of \(\mathrm{Al}(\mathrm{OH})_{3}\) . The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.107 g. What is the mass percent of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) in the sample?

Short Answer

Expert verified
The mass percent of $\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}$ in the mixture is 32.34%.

Step by step solution

01

Find the moles of Al(OH)₃

First, we need to find the number of moles of Al(OH)₃ precipitate formed. For this, we can use the mass of the precipitate and the molar mass of Al(OH)₃. The molar mass of Al(OH)₃ is: M_Al(OH)₃ = 27.0 g/mol (Al) + 3*(16.0 g/mol (O) + 1.0 g/mol (H)) = 27.0 + 3*(17.0) = 27.0 + 51.0 = 78.0 g/mol Now, we can find the moles of Al(OH)₃ formed: moles_Al(OH)₃ = mass_Al(OH)₃ / M_Al(OH)₃ = 0.107 g / 78.0 g/mol = 0.00137 mol
02

Find the moles of Al₂(SO₄)₃

Since every mole of Al(OH)₃ is formed from one mole of Al₂(SO₄)₃ in the reaction, the number of moles of Al₂(SO₄)₃ in the sample is equal to the moles of Al(OH)₃: moles_Al₂(SO₄)₃ = moles_Al(OH)₃ = 0.00137 mol
03

Calculate the mass of Al₂(SO₄)₃

Now we can find the mass of Al₂(SO₄)₃ in the sample using the number of moles and molar mass of Al₂(SO₄)₃. The molar mass of Al₂(SO₄)₃ is: M_Al₂(SO₄)₃ = 2*27.0 g/mol (Al) + 3*(4*16.0 g/mol (O) + 32.1 g/mol (S)) = 54.0 + 3*(64.0 + 32.1) = 54.0 + 3*(96.1) = 54.0 + 288.3 = 342.3 g/mol Now, let's calculate the mass: mass_Al₂(SO₄)₃ = moles_Al₂(SO₄)₃ * M_Al₂(SO₄)₃ = 0.00137 mol * 342.3 g/mol = 0.469 g
04

Find the mass percent of Al₂(SO₄)₃ in the mixture

Finally, we can calculate the mass percent of Al₂(SO₄)₃ in the mixture using the mass of Al₂(SO₄)₃ and the mass of the sample: mass_percent_Al₂(SO₄)₃ = (mass_Al₂(SO₄)₃ / mass_sample) * 100% = (0.469 g / 1.45 g) * 100% = 32.34% The mass percent of Al₂(SO₄)₃ in the mixture is 32.34%.

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

Triiodide ions are generated in solution by the following (unbalanced) reaction in acidic solution: $$\mathrm{IO}_{3}^{-}(a q)+\mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{3}^{-}(a q)$$ Triodide ion concentration is determined by titration with a sodium thiosulfate \(\left(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\right)\) solution. The products are iodide ion and tetrathionate ion \(\left(\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\right)\) a. Balance the equation for the reaction of \(\mathrm{IO}_{3}^{-}\) with \(\mathrm{I}^{-}\) ions. b. A sample of 0.6013 g of potassium iodate was dissolved in water. Hydrochloric acid and solid potassium iodide were then added. What is the minimum mass of solid KI and the minimum volume of 3.00 M HCl required to convert all of the 1 \(\mathrm{O}_{3}^{-}\) ions to \(\mathrm{I}_{3}^{-}\) ions? c. Write and balance the equation for the reaction of $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\( with \)\mathrm{I}_{3}-$ in acidic solution. d. A 25.00 -mL sample of a 0.0100\(M\) solution of \(\mathrm{KIO}_{3}\) is reacted with an excess of \(\mathrm{KL}\) . It requires 32.04 \(\mathrm{mL}\) of \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution to titrate the \(\mathrm{I}_{3}^{-}\) ions present. What is the molarity of the \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) solution? e. How would you prepare 500.0 \(\mathrm{mL}\) of the KIO\(_{3}\)solution in part d using solid \(\mathrm{KIO}_{3} ?\)

A mixture contains only NaCl and \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) . A \(0.456-\mathrm{g}\) sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of \(\mathrm{Fe}(\mathrm{OH})_{3}\) . The precipitate is filtered, dried, and weighed. Its mass is 0.107 \(\mathrm{g}\) . Calculate the following. a. the mass of iron in the sample b. the mass of Fe(NO \(_{3} )_{3}\) in the sample c. the mass percent of \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) in the sample

Balance the following oxidation–reduction reactions that occur in basic solution. a. $\mathrm{Cr}(s)+\mathrm{CrO}_{4}^{2-}(a q) \rightarrow \mathrm{Cr}(\mathrm{OH})_{3}(s)$ b. $\mathrm{MnO}_{4}^{-}(a q)+\mathrm{S}^{2-}(a q) \rightarrow \mathrm{MnS}(s)+\mathrm{S}(s)$ c. $\mathrm{CN}^{-}(a q)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{CNO}^{-}(a q)+\mathrm{MnO}_{2}(s)$

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. \(\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \rightarrow\)

Assign oxidation states for all atoms in each of the following compounds. a. $\mathrm{UO}_{2}^{2+} \quad \quad f. \mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}$ b. $\mathrm{As}_{2} \mathrm{O}_{3} \quad \quad g. \mathrm{Na}_{2} \mathrm{P}_{2} \mathrm{O}_{3}$ c. \(\mathrm{NaBiO}_{3} \quad h. \mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. $\mathrm{As}_{4} \quad\quad \quad i. \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ e. \(\mathrm{HAsO}_{2}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

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