Solutions

Solute

The minor component in a solution dissolved in solvent

solvent

the major component in a solution usally the liquid in which a solute is dissooved in

solution

a liquid mixture in which the solute is uniformly distrubted within the solovent

unsaturated

less than the maximum of solute is dissolved in solvent or more stuff can still be dissolved

Saturated

The maximum amount of a solute is dissolved in a solvent resulting in a precipitate at the bottom

Soluble Salts

Group 1 Metal Cations

No3-

ClO4-

C2H3O2-

NH4+

Insouble Salts

Ag+

Pb2+

Hg2+

OH-

S2-

CO3 -2

PO4 -3

Soluble trump the Insoluble meaning

if you have one soluble one insoluble the soluble will win out

Electrolytes

Substance that have a nautral positive or negative electral charge when dissolved in water

Strong Electrolytes

fully dissoacciate in water

type of strong electrolytes

soluble ionic compounds

strong acids

strong bases

Weak Electrolytes

Weak Acids

Weak Bases

Non electrolytes

arent acidic or basic

Solubility rules for solids

solids are more soluble at higher temp

solubility rules for gases

gases are more soluble at lower temps

solubility rules for gases 2

gases are more soluble at higher pressure

Spectrophotometry

When light passes through a solution measure how much light is sent in and comes out

Beers Law of Spectrophotometry

Light absorption is directly proportional to path length and conc of solution

beer law equation

A = E l C

A = absorbance

E = Molar Absorbivity

l = path length (cm)

c = conc of soltuoon

What does beer law shwo

more concentration solution absorb more lght than a diluted solution

Polar Charge

A seperation of electric charge leading to a dipole from different electronegativity

Like Dissolves like means

Polar dissolve polar

Non polar dissolve non polar

non polar can not dissolve polar

Class of Matter

Pure substance or mixture

element

a substance consisting of one type of atom and no longer broken down

compound

a pure chemical made up of two or more different elements`

heterogenous mixture

particles distrubited non uniformly

can be physically seperated

homogenous

particles distrubted uniformly

cannot be physically seperated

Molarity

Number of Moles per one liter of solution M

Molaliity

the number of moles of solute per 1 kg of solvent

Molarity equation

moles solute/ Liter of solution M

Molality equation

moles of solute / kg of solvent

Dilution

Process of reducing the concentration of a solute in solution

How to calculate volume of solution after a dilution

M1V1 = M2V2

Diluted Solution

has very little solute and can a dissolve a lot more solute

Concentrated Solution

Has a lot more solute and can dissolve a little more soluteS

Saturated Solution

Maximum amount of solute and cannot dissolve anymore solute

Normality

N = n x M

N = normality

n = number of equivalents

Mol Fraction

The ratio of number of moles of one component of mixture to the toal number of moles

Mol Fraction Equation

moles A /Total Moles

Colligative

Properties that depend upon the concentration of solute moleucles but not upon the identy of the solute

Non Colligative

properties that depend on the identity of the dissolved species and solvent

Non Colligative Properties Examples

Surface Tenson

Viscosity

Solubility

Color and Density

Colligative Properties examples

Vapor-Pressure Depression

Boilibng Point

where the vapor pressure = atmospheric pressure

liquid to gas

Boiling point at higher altitutdes means

As elevation increases atmospheric pressure decreases and therefore lower vapor pressure and lower boiling point

Boiling point at low altiltude levels

elevation decrease pressure increase and vapor pressure increase and therefore boiling point increases

Vapor Pressure Depression

Vapor pressure of a pure solvent is greater than the vapor pressure of a soltuion

As vapor pressure increases what happens to boiling point

decrease in boiling point

What happens when we add solute to vapor pressure

the boiling point increases R

Raoults Law

Pa = Xa * P A

Pa = vapor pressure

Xa = Mol Fraction

P A = pure vapor pressure of solvent

Boiling Point Elevation Equation

Delta Tb = kb im

Delta TB = amount of bp increases

kb = solvent bp elevation constnat

i = Van Hoff Factor

m = molal concentration fo solution

Freezing Point Depression Equation

Delta Tf = -kf I m

Osmotic Pressure

the pressure it would take to stop osmosis from happening

Osmotic Pressure Equation

Osmotic pressure = iMRT

Ionic Equation Definiton

Equations in which ionic compounds are written as speertead ions

Spectator Ions

Ions that do not take part in the reaction and found in both before and after

Net Ionic Equation

only shows the elements directly involved in the reaciton