Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 16

Indicate the principal type of solute-solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute- solvent interaction: (a) KCl in water, (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right),(\mathbf{c})\) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water.

Short Answer

Expert verified
The principal types of solute-solvent interactions for the given solutions are: (a) Ion-dipole interaction for KCl in water, (b) Dispersion forces for \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene, and (c) Dipole-dipole interaction for methanol in water. The ranking of the solutions based on the strength of solute-solvent interactions is: Weakest - (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene, Medium - (c) Methanol in water, and Strongest - (a) KCl in water.

Step by step solution

01

Identify Types of Solute-Solvent Interactions

There are mainly three types of solute-solvent interactions: 1. Ion-dipole interactions: Occur between ions and polar molecules 2. Dipole-dipole interactions: Occur between polar molecules 3. Dispersion forces: Occur between non-polar molecules
02

Analyze the Given Solutions

We will analyze each of the given solutions to determine the type of solute-solvent interaction: (a) KCl in water: KCl is an ionic compound and water (H2O) is a polar molecule. Therefore, the interaction is an ion-dipole interaction. (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\): Both solute (\(\mathrm{CH}_{2} \mathrm{Cl}_{2}\)) and solvent (benzene) are non-polar molecules. Therefore, the interaction is due to dispersion forces. (c) Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water: Both methanol and water are polar molecules. Therefore, the interaction is a dipole-dipole interaction.
03

Rank the Solutions Based on Strength of Interactions

Ion-dipole interactions are generally stronger than dipole-dipole interactions, which in turn are stronger than dispersion forces. Therefore, the order of strength of solute-solvent interactions is: Weakest: (b) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) in benzene (Dispersion forces) Medium: (c) Methanol in water (Dipole-dipole interactions) Strongest: (a) KCl in water (Ion-dipole interaction)

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

(a) What is the molality of a solution formed by dissolving 1.12 mol of KCl in 16.0 mol of water? (b) How many grams of sulfur \(\left(\mathrm{S}_{8}\right)\) must be dissolved in \(100.0 \mathrm{~g}\) of naphthalene $\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\( to make a \)0.12 \mathrm{~m}$ solution?

What is the osmotic pressure formed by dissolving \(50.0 \mathrm{mg}\) of acetylsalicylic acid $\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)\( in \)0.100 \mathrm{~L}\( of water at \)37^{\circ} \mathrm{C} ?$

Compounds like sodium stearate, called "surfactants" in general, can form structures known as micelles in water, once the solution concentration reaches the value known as the critical micelle concentration (cmc). Micelles contain dozens to hundreds of molecules. The cmc depends on the substance, the solvent, and the temperature. At and above the \(\mathrm{cmc}\), the properties of the solution vary drastically. (a) The turbidity (the amount of light scattering) of solutions increases dramatically at the \(\mathrm{cmc}\). Suggest an explanation. (b) The ionic conductivity of the solution dramatically changes at the \(\mathrm{cmc}\). Suggest an explanation. (c) Chemists have developed fluorescent dyes that glow brightly only when the dye molecules are in a hydrophobic environment. Predict how the intensity of such fluorescence would relate to the concentration of sodium stearate as the sodium stearate concentration approaches and then increases past the \(\mathrm{cmc}\).

Describe how you would prepare each of the following aqueous solutions: \((\mathbf{a}) 1.50 \mathrm{~L}\) of $0.110 \mathrm{M}\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}$ solution, starting with solid $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} ;(\mathbf{b}) 225 \mathrm{~g}\( of a solution that is \)0.65 \mathrm{~m}\( in \)\mathrm{Na}_{2} \mathrm{CO}_{3},\( starting with the solid solute; \)(\mathbf{c}) 1.20$ \(\mathrm{L}\) of a solution that is $15.0 \% \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}$ by mass (the density of the solution is \(1.16 \mathrm{~g} / \mathrm{mL}\) ), starting with solid solute; (d) a \(0.50 \mathrm{M}\) solution of \(\mathrm{HCl}\) that would just neutralize \(5.5 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) starting with $6.0 \mathrm{MHCl}$.

At ordinary body temperature \(\left(37^{\circ} \mathrm{C}\right),\) the solubility of \(\mathrm{N}_{2}\) in water at ordinary atmospheric pressure is \(0.015 \mathrm{~g} / \mathrm{L}\) Air is approximately $78 \mathrm{~mol} \% \mathrm{~N}_{2}$. (a) Calculate the number of moles of \(\mathrm{N}_{2}\) dissolved per liter of blood, assuming blood is a simple aqueous solution. (b) At a depth of $30.5 \mathrm{~m}\( in water, the external pressure is \)405 \mathrm{kPa}$. What is the solubility of \(\mathrm{N}_{2}\) from air in blood at this pressure? (c) If a scuba diver suddenly surfaces from this depth, how many milliliters of \(\mathrm{N}_{2}\) gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

Read Explanation

Organic 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