Q: Which of the following is the correct formula for calculating molarity ($$M) of a $$solution?

$$M = \frac{\text{moles of solute (mol)}}{\text{volume of solution (L)}}$$

Question 1

Which type of intermolecular force is depicted in the first image with blue (+) and yellow (–) spheres, and what is the primary basis of attraction for this force?

Accepted Answer

Ion-ion; attraction between oppositely charged ions

Question 2

Refer to the diagram showing 'Ion-induced dipole' and 'Dipole-induced dipole' interactions. Which of the following best describes a dipole-induced dipole force?

Accepted Answer

Attraction between a polar molecule and a nonpolar molecule due to induced polarity

Question 3

The image with Cl⁻ and hexane (C₆H₁₄) illustrates which type of intermolecular force?

Accepted Answer

Ion-induced dipole

Question 4

Which statement about dispersion (London) forces is correct based on the provided images and tables?

Accepted Answer

Dispersion forces increase with molecular size and are present in all substances.

Question 5

According to the table comparing CH₄, C₈H₁₈, and C₃₆H₇₄, what trend is observed as molecular size increases?

Accepted Answer

Melting point and boiling point both increase due to stronger dispersion forces.

Question 6

Given the two molecular models of n-pentane and neopentane, which has the higher boiling point and why?

Accepted Answer

n-Pentane, because its elongated shape allows more intermolecular contact and stronger dispersion forces.

Question 7

Which intermolecular force is the strongest according to the table with energy values, and what is a typical energy range for this force?

Accepted Answer

Ion-ion; 40–600 kJ/mol

Question 8

Which of the following best explains why NaCl dissolves in water, as shown in the image with Na⁺ and Cl⁻ surrounded by water molecules?

Accepted Answer

Water molecules surround and stabilize the ions through ion-dipole interactions.

Question 9

Which solution will conduct electricity most effectively, as shown in the images with a light bulb and electrodes?

Accepted Answer

A solution of NaCl

Question 10

Which of the following best describes the Tyndall effect, as illustrated by the images with light scattering in colloids?

Accepted Answer

The scattering of light by particles in a colloid, making the path of light visible

Question 11

A 12.0% (w/w) glucose solution contains 435 g of solution. What is the mass of glucose present?

Accepted Answer

$$52.2\ \mathrm{g}$$

Question 12

Which of the following is a colloid, based on the provided tables and images?

Accepted Answer

Milk

Question 13

Which of the following best explains why hexane and water do not mix, as shown in the molecular diagram?

Accepted Answer

Hexane is nonpolar and cannot form hydrogen bonds with water.

Question 14

Which vitamin would be most likely to accumulate to toxic levels in the body if consumed in excess, based on solubility properties?

Accepted Answer

Vitamin A

Question 15

Which of the following best describes the relationship between molecular structure and solubility in water?

Accepted Answer

The more atoms that can participate in hydrogen bonding, the higher the solubility in water.

Question 16

Which of the following is the correct formula for calculating molarity ($$M) of a $$solution?

Accepted Answer

$$M = \frac{	ext{moles of solute (mol)}}{	ext{volume of solution (L)}}$$

Question 17

If you want to prepare 1.0 L of a 0.15 M NaOH solution from a 6.0 M NaOH stock solution, how much of the stock solution should you use?

Accepted Answer

$$0.025\ \mathrm{L}$$

Question 18

Which of the following best describes an unsaturated solution?

Accepted Answer

A solution that contains less solute than the maximum amount that can dissolve at a given temperature

Question 19

Which factor increases the solubility of gases in liquids?

Accepted Answer

Increasing pressure

Energy and Physical Properties: Intermolecular Forces, Solutions, and Concentration

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