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Diluting a solution Amount of moles of solute before dilution Amount of moles of solute after dilution = c D V D = c C V C Practice problems: p. 321 # p. 326 # 18, 19
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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.