Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 11: Q11.1-9E (page 646)

Explain why the ions \(N{a^ + }\) and \(C{l^ - }\) are strongly solvated in water but not in hexane, a solvent composed of nonpolar molecules.

Short Answer

Expert verified

Solvated means stabilizing both\(N{a^ + }\)and\(C{l^ - }\)

Step by step solution

01

Solvated

Water is a polar solvent and high dipole moment. \(N{a^ + }\)interacts with oxygen and \(C{l^ - }\)interacts with hydrogen in a water solvent. This process is called solvated.

02

 Step 2: Nonpolar

Hexane is a nonpolar solvent and the dipole moment is zero. So that, it does not take place any interaction in between hexane and \(N{a^ + }\)\(C{l^ - }\)ions.

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 molality of each of the following solutions:

  1. 583 g of \({{\bf{H}}_{\bf{2}}}{\bf{S}}{{\bf{O}}_{\bf{4}}}\) in 1.50 kg of water—the acid solution used in an automobile battery
  2. 0.86 g of NaCl in 1.00 × 102 g of water—a solution of sodium chloride for intravenous injection
  3. 46.85 g of codeine, \({{\bf{C}}_{{\bf{18}}}}{{\bf{H}}_{{\bf{21}}}}{\bf{N}}{{\bf{O}}_{\bf{3}}}\), in 125.5 g of ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\)
  4. 25 g of I2 in 125 g of ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\).

Calculate the mole fractions of methanol, \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\); ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\); and water in a solution that is 40% methanol, 40% ethanol, and 20% water by mass. (Assume the data are good to two significant figures.)

The triple point of air-free water is defined as 273.15 K. Why is it important that the water be free of air?

When \({\bf{KN}}{{\bf{O}}_{\bf{3}}}\) is dissolved in water, the resulting solution is significantly colder than the water was originally.

  1. Is the dissolution of \({\bf{KN}}{{\bf{O}}_{\bf{3}}}\) an endothermic or an exothermic process?
  2. What conclusions can you draw about the intermolecular attractions involved in the process?
  3. Is the resulting solution an ideal solution?

Which of the following gases is expected to be most soluble in water? Explain your reasoning.

(a) \({\bf{CH}}_4\)

(b) \({\bf{CCl}}_4\)

(c)\({\bf{CHCl}}_3\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

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