Chemistry - colligative properties and conversions

Boiling point

The temperature at which a liquid is converted into a gas.

Colligative property

Dependant on how much of something is dissolved in a solvent (water), opposed to the identity of what is dissolved in that solution.

Dilute solutions of the same concentration

same boiling point.

Concentration

removal of a solvent, increases concentration

Dilution

addition of a solvent, decreases concentration

Adding solute particles to a solution

boiling point elevates

Pure water boiling point

100C at 1atm (1 atmospheric pressure)

Add salt to water

Freezing point decreases

Vapor pressure

How quickly/completely a liquid evaporates

Strong intermolecular forces

lowers the vapor pressure

Make it harder for surface molecules to escape

vapor pressure

Strong intermolecular forces

higher boiling point

Table salt boiling point

1465C but water doesn’t need that much to boil (when salt is added)

Solute particles

decreases vapor pressure

Mol/volume

22.4L/mol

Mol/mass

GFM/mol

Mol/particle

6.02 times 10²³

Moles to x

multiply

x to moles

divide

Moles formula

Moles = Mass/GFM

Grams formula

Grams = moles x GFM

Particles formula (atoms or molecules)

Particles = Moles x 6.02×10²³

Particles to moles

Moles = Given particles X 6.02×10²³