Ch.12 - SolutionsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: In which solvent do you expect hexane (C6H14) to be miscible? A. CH3CNB. C5H12C. CH3COOHD. CH3OHE. H2O

Problem

In which solvent do you expect hexane (C6H14) to be miscible? 

A. CH3CN

B. C5H12

C. CH3COOH

D. CH3OH

E. H2O

Solution

We’re being asked in which solvent do we expect hexane (C6H14) to be miscible. Recall that the main idea in dissolution is like dissolves like, which means compounds with the same polarity and intermolecular force can dissolve each other.


Hexane is an example of a hydrocarbon, a compound composed only of carbons and hydrogens. Hydrocarbons are nonpolar compounds. This means that hexane is a nonpolar molecule that exhibits dispersion forces.


So for this, we need to draw the Lewis structures of the given choices and determine their polarity.


Step 1: Determine the central atom in this molecule.

Step 2: Calculate the total number of valence electrons present and draw the Lewis structure for the molecule.

Step 3: Determine the polarity of the molecule.


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