Diluting a solution Amount of moles of solute before dilution Amount of moles of solute after...

g /1 0 0 m L (m /v) %(m /m )%(v/v)%

p p mp p b

m ol/Lc= n /V

C on c en tra tion

d ep en d s on> tem p era tu re

> ag ita t ion> p art ic le s iz e

R a te o f d iss o lvin g

d ep en d s on>m olec u le s ize> tem p eratu re

>p res su re

Ion ic c om p ou n d s d iss o lvein p o la r s o lven ts

(eg . N aC l in H 2 O )

Ion -d ip o le a ttrac tion

P ola r c ova len t c om p ou n d sd iss o lve in p o la r so lven ts

eg . s u g ar in w a ter

d ip o le-d ip o le a ttrac t ion

N on p o la r c om p ou n d sd is so lve in n on -p o la r s o lven ts

(eg . o il in b en zen e )

n o p o lar o r ion ic a ttrac tion

A ttrac t ion b etw een p art ic les

S olu b ility(g /1 0 0 m L )(h ow m u ch so lu te d isso lves )

S o lu t ion sso lid (eg . s tee l)liq u id (eg . ju ice )

g as (eg . a ir)

Diluting a solutionAmount of moles of

solute before dilutionAmount of moles of solute after dilution

=

cDVD = cCVC

Practice problems: p. 321 # 25-27 p. 326 # 18, 19

Solubility Rules Song (by C. Watt) The thing about solubility that is great,It will always dissolve if it is a nitrate. Something else that is helpful for you and IIt will be soluble if it is ammonium or an alkali. When I think about chlorides, bromides, and iodides, it hurts

my headBecause they are soluble, except with silver, mercury and lead It gets a lot harder, with sulfates, its trueIt’s soluble, except with calcium, strontium, barium, radium,

and lead, which all have a charge of plus two. Now there had to be the insolubles, they cannot hideExcept with cations from #2, carbonate, phosphate, and

hydroxide.

Using solubility rules to …1. Predict whether a salt is soluble or insoluble. 2. Predict the formation of a precipitate.3. Write the net ionic equation

Ionic DissociationDefinition: dissolving of ionic substances in

which ions separate from each other and the crystal

Examples:NaCl (s) Na+(aq) + Cl-(aq)Na2SO4(s) 2Na+(aq) + SO4

2-(aq)(NH4)3PO4(s) 3NH4

+(aq) + PO43-(aq)

Solution Stoichiometry 1. Write a balanced chemical equation. 2. Determine the number of moles of the

reactants. You will need to use: c=n/V and n=m/M

3. Determine the limiting reagent. 4. Use the limiting number of moles in a

ratio to find unknowns. 5. Convert back from moles to mass

Property Acids BasesTaste sour bitter

Electrical Conductivity

Conducts electricity

Conducts electricity

Feel of solution

No characteristi

c feel

Feel slippery

Reaction with litmus

paper

Turn litmus paper red

Turn litmus paper blue

Reaction with active

metals

Produce hydrogen

gas

Do not react

Reaction with

carbonates

Produce CO2 Do not react

Arrhenius vs Bronsted-Lowry

ArrheniusAcid Any substance that

dissociates to form H+ in aqueous solution

BaseAny substance that

dissociates to form 0H- in aqueous solution

Bronsted-LowryAcidAny substance that

provides a proton to another substance

BaseAny substance that

receives a proton from an acid

Conjugate Acid-Base PairsHBr(aq) + H20(l) -> H30+(aq) + Br-

(aq)

Acid – gives up a proton (H) {HBr(aq) }Base – accepts a proton (H){H20(l) }Conjugate base – particle that has lost the

proton. {Br-(aq)}Conjugate acid – particle that has gained a

proton {H30+(aq) }

Calculating pH

pH = -log[H3O+]

Neutralization Reactions1. Reaction between an acid and a base produces

an ionic compound (a salt) and water acid + base -> a salt + water

2. Reaction between an acid and a carbonate produces an ionic compound, water and carbon dioxide

Acid + carbonate -> carbon dioxide + water + ionic salt

Calculations involving neutralization reactions1. Write the balanced equation.2. Calculate the number of moles of given acid

or base.3. Determine the number of moles of acid or

base needed. (use mole ratio if necessary).4. Calculate the final concentration of the

required acid or base.