Question

Determine if each pair of compounds forms a homogeneous solution when combined. For those that form homogeneous solutions, indicate the type of forces that are involved.

a. CCl₄ and H₂O
b. CH₃CH₂OH and H₂O
c. NaCl and H₂O
d. Br₂ and C₆H₆

Answer 1

CCl₄ and H₂O do not form a homogeneous solution due to polarity differences. CH₃CH₂OH (ethanol) and H₂O form a homogeneous solution with hydrogen bonding. NaCl and H₂O also form a homogeneous solution through ion-dipole interactions, and Br₂ and C₆H₆ form a solution due to London dispersion forces.

Step-by-step explanation:

The question asks us to determine if various pairs of compounds will form a homogeneous solution when combined and to indicate the type of forces involved for those that do. Here are the answers for each pair:

• CCl₄ and H₂O: These do not form a homogeneous solution, because CCl₄ is nonpolar and water (H₂O) is polar. The forces between like molecules (water-water and CCl₄-CCl₄) are stronger than between unlike molecules (CCl₄-water).
• CH₃CH₂OH (ethanol) and H₂O: These form a homogeneous solution. The main intermolecular force involved is hydrogen bonding, as both ethanol and water can form hydrogen bonds.
• NaCl and H₂O: These form a homogeneous solution. The ionic compound NaCl dissolves in water due to the ion-dipole interactions between the ions and the polar water molecules.
• Br₂ and C₆H₆ (benzene): These form a homogeneous solution. Both bromine and benzene are nonpolar, so the intermolecular forces are London dispersion forces.