Chemistry second trimester

Homogeneous mixtures of two or more substances
Contains a solute, usually in a smaller quantity, uniformly dispersed in another substance called the solvent

Can't be separated by filtration
Can be separated by evaporation
Can give color to a solution

Polar
The most common solvent

Polar disolves in polar
Non polar disolves in non polar

On the surface of a NaCl crystal are atracted to polar water molecules

In solution are hydrated by H2O molecules that surround each ion

Attractive forces occur between solute and solvent particles when the solute and solvent are similar in polarity

"Like dissolves like"

Hydration separates the ions

Oils iodine, grease the non the
There are no attractions between polar solute and polar solvent
Non polar molecules will forma solution with nonpolar solvents

Electrolyte solutes
Non electrolyte solutes

They completely dissociated (break up) into ions- forming a solution that conducts electricity.

They dond dissociate into ions, but break up into molecules, forming a solution that does not conduct electricity.

Strong electrolyte
Weak electrolyte

Completely dissociate
Produce ions
Conduct an electric current
For example 100% ions
Salt dissolving in water

Dissolve mostly as molecules
Produce a few ions
Conduct a weak current
For example NH3 gas reaction

Dissolve as molecules
Do not produce ions
Do not conduct a current
For example carbon compounds like methanol, ethanol, urea

It is the maximum amount of solute that dissolves in a specific amount of solvent.
Can be expressed as grams of solute per 100 grams of solvent usually water
G of solute / 100 g of water

Unsaturated
Saturated
supersaturated/oversaturated

Under max solubility

Maximum solubility

Over max solubility

Solubility depends on temperature
Increases as temperature increases for most solids
Decreases astemperature increases for gases.

Mass /mass % (m/ m) = mass solute / mass solution x 100
Mass solution = mass solutes + mass solvent

Volume solute / volume solution x100
Vsolution = v solute + v solvent

Grams solute/ ml solution x 100

M = moles of solute/ l solution

M= moles solute/ kg solvent

C1 V1= C2 V2