Intermolecular Forces and Properties

It absorbs heat from surroundings raising roads' temperature above freezing point.

It chemically reacts with ice forming compounds that melt at higher temperatures than pure ice.

It disrupts hydrogen bonding between water molecules, lowering its freezing temperature (freezing point depression).

Salt provides nucleation points for ice crystals preventing their formation even below normal freezing point of water.

Molecules structurally similar with atomic charge distribution resulting in nearly equal rates of evaporation

The unsaturated hydrocarbon due to less effective London dispersion forces than those present in the halogenated counterpart

The halogenated hydrocarbon since polarizability of atoms increases strength of dispersion forces between molecules

Both liquids will evaporate similarly fast because their molecular mass impacting volatility

London dispersion force dominant liquid, such as bromine (Br2)

Dipole-dipole interacting liquid, such as chloroform (CHCl3)

Hydrogen bond forming liquid, such as water (H2O)

Nonpolar molecular solid, such as iodine (I2)

More solvent molecules interact with salt ions, quickly dissolving additional salt.

No new salt dissolves, the added amount settles out.

Salt concentration decreases causing more solvent particles to evaporate.

Added salt immediately precipitates without interacting with solution.

Increasing concentration enhances conductivity due to greater availability of charge carriers from ionized acetic acid.

Concentration changes do not affect conductivity because acetic acid dissociates completely regardless of dilution or concentrating.

Reducing concentration improves conductivity by decreasing dipole-dipole interactions between acetic acid molecules.

Increasing concentration reduces conductivity since excess charge carriers lead to electron-pair recombination before charge transfer.

Exothermic

Kinetic energy

Endothermic

Activation energy

At higher temperatures, saturation concentration universally declines for all types of solutions.

Temperature has no influence over gaseous solutions but affects liquids exclusively.

Saturation concentration remains constant regardless of temperature changes.

It tends to increase saturation concentration for most solid solutes but decrease gas solubility.

Composite material

Chemical compound

Homogeneous mixture

Heterogeneous mixture

The density of the water since it becomes less dense with more dissolved salt.

The boiling point remains static as it will not shift until salting-out occurs.

The mass of water specifically allocated to solvating each ion of salt.

The intrinsic hydrogen bonding between water molecules.

1.20 x 10^22 particles

0.100 particles

6.02 x 10^23 particles

6.02 x 10^21 particles