Solutions - Chapter 12

Chemistry

Solution equilibrium

Solution equilibrium

when dissolving and crystallization take place simultaneously at the same rate

Miscible

two liquids mix with one another (like water and acetic acid making vinegar)

Nonelectrolyte

a substance that dissolves in water to give a solution that will NOT conduct an electric current

Solution

another name for a homogeneous mixture

Suspension

Orange juice with all the pulp settling at the bottom of the glass

Unsaturated

100 grams of water will dissolve 34.2g of KCl at 20 degrees C, but you only dissolve 34.0g

Henry’s Law example

this explains why sodas are bottled under pressure

Hydration

when water is added to make a solution

Alloy

14 Karat gold is an example

Solvent

in 14 Karat gold it is the gold (not the added silver or copper)

Heat of Solution

energy being absorbed (or released) when a solute dissolves in a given amount of solvent

Supersaturated

100g of H2O will dissolve 162g of KI at 40 degrees C. you get 171g to dissolve by heating and cooling it

Colloid

a mixture with particles not too big or not too small, they are just right (intermediate in size)

Solvation

process that describes a solute particle being surrounded by solvent

Saturated

Maximum amount of a substance that will dissolve at a certain temperature

Solute

in ocean water, it is the salt

Tyndall Effect

a beam of light coming thru a window and seeing dust particles floating in it is an example

Electrolyte

these solutions have a LOT of ions in solution and will conduct electricity

Immiscible

oil and vinegar salad dressing are an example

Effervescence

all the delicate bubbles that rise to the surface when you open the soda or pour the soda

Brownian Motion

random motion due to collisions of rapidly moving particles (example: colloid particles detected through a microscope)

Particle size: solution

.01-1 nm

Particle size: colloid

1-1000 nm

Particle size: suspension

over 1000 nm

Examples of a Solution

oxygen in nitrogen, alcohol in water, sugar in water

Examples of a Colloid

aerosol (liquid or solid dispersed in a gas), smoke, fog, mist, paint, milk, mayo

Examples of a Suspension

flour in water, mud in water

(+) Heat of Soln

endothermic: as temp increases, solubility increases (most solids)

(-) Heat of Soln

exothermic: as temp increases, solubility decreases

requires energy/endothermic

solvent particles must move apart to allow the solute to enter the liquid

energy released/exothermic

solute particles are attracted to solvent particles

Henry’s Law

solubility of a nonvolatile gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

Gases:

as temp increases, solubility would decrease; as pressure increases, solubility would increase

concentrated

solute proportion > solvent

dilute

solute proportion < solvent

concentration of solutions

a measure of the amount of solute in a given amount of solvent

% by mass

mass solute/mass solution x100

molarity

moles solute/L solution

molality

moles solute/kg solvent

dilution equation

M1V1 = M2V2