Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Problem 44

Which solvent, water or hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right),\) would you choose to dissolve each of the following? a. \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) b. \(\mathrm{CS}_{2}\) c. \(\mathrm{CH}_{3} \mathrm{OH}\) d. \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{CH}_{2} \mathrm{OH}\) e.\(\mathrm HCl\) {f .} \( \mathrm{C}_{6} \mathrm{H}_{6}\)

Short Answer

Expert verified
a. Water b. Hexane c. Water d. Hexane e. Water f. Hexane

Step by step solution

01

Identifying compound polarity

Copper nitrate, Cu(NO3)2, is an ionic compound because it consists of a metal (Cu) and a polyatomic ion (NO3−). Ionic compounds are generally considered to be polar.
02

Choosing the appropriate solvent

Since Cu(NO3)2 is polar, it will dissolve better in the polar solvent water than in the nonpolar solvent hexane. #b. CS2#
03

Identifying compound polarity

Carbon disulfide, CS2, is a nonpolar compound as the electronegativity difference between carbon and sulfur is small.
04

Choosing the appropriate solvent

Since CS2 is nonpolar, it will dissolve better in the nonpolar solvent hexane than in the polar solvent water. #c. CH3OH#
05

Identifying compound polarity

Methanol, CH3OH, is a polar compound because the oxygen atom forms a polar bond with the hydrogen atom due to their significant electronegativity difference.
06

Choosing the appropriate solvent

Since CH3OH is polar, it will dissolve better in the polar solvent water than in the nonpolar solvent hexane. #d. CH3(CH2)16CH2OH#
07

Identifying compound polarity

This molecule, which is a long-chain alcohol, is largely nonpolar because it consists of a long hydrocarbon chain. The hydroxyl group at the end of the molecule is polar, but its contribution to the overall polarity of the molecule is fairly small due to the size of the hydrocarbon chain.
08

Choosing the appropriate solvent

Since the hydrocarbon chain dominates the overall polarity of the molecule, it is considered more nonpolar than polar. Therefore, it will dissolve better in the nonpolar solvent hexane than in the polar solvent water. #e. HCl#
09

Identifying compound polarity

Hydrogen chloride, HCl, is a polar compound due to the significant electronegativity difference between hydrogen and chlorine atoms.
10

Choosing the appropriate solvent

Since HCl is polar, it will dissolve better in the polar solvent water than in the nonpolar solvent hexane. #f. C6H6#
11

Identifying compound polarity

Benzene, C6H6, is a nonpolar compound as it consists of a symmetrical ring of carbon and hydrogen atoms that create an overall equal distribution of electron density.
12

Choosing the appropriate solvent

Since C6H6 is nonpolar, it will dissolve better in the nonpolar solvent hexane than in the polar solvent water.

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

Calculate the molarity and mole fraction of acetone in a \(1.00-m\) solution of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}\right)\) in ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right) .\) (Density of acetone \(=0.788 \mathrm{g} / \mathrm{cm}^{3} ;\) density of ethanol \(=0.789\) \(\mathrm{g} / \mathrm{cm}^{3} .\) ) Assume that the volumes of acetone and ethanol add.

A \(4.7 \times 10^{-2}\) mg sample of a protein is dissolved in water to make \(0.25 \mathrm{mL}\) of solution. The osmotic pressure of the solution is 0.56 torr at \(25^{\circ} \mathrm{C}\). What is the molar mass of the protein?

You make \(20.0 \mathrm{g}\) of a sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) and NaCl mixture and dissolve it in \(1.00 \mathrm{kg}\) water. The freezing point of this solution is found to be \(-0.426^{\circ} \mathrm{C}\). Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.

In lab you need to prepare at least \(100 \mathrm{mL}\) of each of the following solutions. Explain how you would proceed using the given information. a. \(2.0 \mathrm{m} \mathrm{KCl}\) in water (density of \(\mathrm{H}_{2} \mathrm{O}=1.00 \mathrm{g} / \mathrm{cm}^{3}\) ) b. \(15 \%\) NaOH by mass in water \(\left(d=1.00 \mathrm{g} / \mathrm{cm}^{3}\right)\) c. \(25 \%\) NaOH by mass in \(\mathrm{CH}_{3} \mathrm{OH}\left(d=0.79 \mathrm{g} / \mathrm{cm}^{3}\right)\) d. 0.10 mole fraction of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in water \(\left(d=1.00 \mathrm{g} / \mathrm{cm}^{3}\right)\)

You and your friend are each drinking cola from separate \(2-\mathrm{L}\) bottles. Both colas are equally carbonated. You are able to drink 1 L of cola, but your friend can drink only about half a liter. You each close the bottles and place them in the refrigerator. The next day when you each go to get the colas, whose will be more carbonated and why?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

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