Solutions - Quartzland
Solutions
1) Solute – the stuff you are interested in
Solvent - that which dissolves the stuff
Solution – the result
Solid/liquid – sugar water
Liquid/liquid – alcohol in water
Gas/liquid – carbon dioxide in water (soda pop)
Solid/solid – gold ring
Liquid/solid – jello
Gas/ solid – pumice stone (??)
Solid/gas – smoke
Liquid gas – fog
Gas/ gas – air
REMEMBER – A solution is a homogeneous mixture. You can vary its composition and you can mechanically separate the components.
2) Solutes can be Slightly Soluble
Soluble
Very soluble
Insoluble – not soluble
Miscible - two liquids that dissolve in each other when they are mixed
(acetic acid in water)
Immiscible - two liquids that do not dissolve in each other when mixed
(vinegar and oil salad dressing)
Emulsion – two liquids that mixed together that are usually immiscible
(mayonnaise)
Emulsifying agent – A substance the links the two immiscible
components together forming an emulsion
(egg whites used to link vinegar and
oil together ( mayonnaise)
REMEMBER – Solubility deals with how much will dissolve.
Conditions that affect solubility include:
a) Temperature goes up ( Solubility of Gas goes down
( Solubility of Solid generally increases
( Solubility of Liquid has little effect
b) Pressure goes up ( Solubility of Gas goes up (can of soda)
( Solubility of Solid has no effect
( Solubility of Liquid has no effect
c) Nature of solute and solvent- “Likes” dissolve “Likes”
Ionic compounds are soluble in polar solvents -
(NaCl in H2O)
Non-polar compounds are soluble in non-polar solvents-
(Grease in gasoline)
3) Rate of solution – How fast a substance will dissolve
a) agitation – stirring dissolves sugar faster in water
b) temperature - sugar dissolves faster in hot water
c) particle size- big particles of sugar dissolve slower
d) concentration - sugar dissolves slower in a solution that
already contain sugar
4) Concentration - How much solute is dissolved in the solution
a) Percent composition
b) Molarity (2.5 M HCl = 2.5 moles HCl/1 Liter solution)
5) Strength – a measure of ability
a) Strong acids- HCl(aq) , HNO3(aq) , H2SO4(aq)
Weak acids – HC2H3O2(aq) , H2CO3(aq) , any other acid
b) Strong bases- NaOH(aq) , KOH(aq)
(metal hydroxides from Group IA)
Weak bases – Al(OH)3(aq) , NH4OH(aq) , any other base
Concentrated Coffee not strong Coffee
Dilute Tea not weak Tea
6) Solution types
a) Unsaturated – solvent can still dissolve more solute
b) Saturated – solvent can not dissolve any more solute
c) Super saturated – Solvent has dissolved more solute than it
normally holds at a given temperature (Honey)
7) Electrolytes – Aqueous solutions that conduct electricity
Strong electrolytes – Strong acids & bases, soluble salts
Weak electrolytes – Weak acids & bases
Non-electrolytes – DI water & toluene (organic compounds)
8) Colligative properties are dependent on the number of particles present
Lowering of the vapor pressure
Lowering of freezing point
Increasing the boiling point
Increasing the osmotic pressure
Osmosis- passage of solvent through a semi-permeable membrane
Osmotic pressure-pressure required to halt the flow of solvent
molecules through a semi-permeable membrane
Reverse osmosis-solvent flows through the semi-permeable
membrane in the reverse direction due to an
increase in the osmotic pressure Living Cells
Isotonic solution- solution on the out-side of a cell has same osmotic
pressure as the inside the cell. No effect
Hypotonic solution – If cell is surrounded by a solution of lower
concentration of solute particles (lower osmotic
pressure), water flows into the cell (plasmolysis)
Hypertonic solution – If cell is surrounded by a solution of higher
concentration of solute particles (higher osmotic
pressure), water flows out of the cell (crenation)
Phase Diagram- H2O
[pic]
Freezing point same as melting point = 0oC for H2O
Boiling point same as condensation point = 100oC for H2O
Boiling point is the temperature where the vapor pressure of a liquid is
equal to the applied pressure.
ΔHfusion = amount of energy required to convert 1.0 gram of stuff from
a solid to a liquid. ΔHfusion H2O = 80 calories /gram.
ΔHvaporization = amount of energy required to convert 1.0 gram of stuff
from a liquid to a gas. ΔHvaporization H2O = 540 calories /gram.
Calorie = amount of energy required to raise the temperature of one
gram of H2O one degree Celsius.
BTU (British Thermal unit) = amount of energy required to raise the
temperature of one pound of H2O one degree Fahrenheit.
Specific Heat (H2O/Solid) = Sp Ht (H2O/Gas) = 0.50 cal/( g x oC)
Specific Heat (H2O/Liquid) = 1.0 cal/( g x oC)
9) Hard water – specifically contains Ca+2, Mg+2 or Fe+3 ions
- precipitates form between these ions and carbonates
Temporary hard water - specifically contains bicarbonate ions (HCO3-1)
- boiling will remove the hardness
Ca(HCO3)2(aq) ( CaCO3(s) + (H2CO3 = H2O(l) + CO2(g) )
10) Soap – a link between polar water and non-polar oil drops
acid + base ( salt + water
Lard + boiled wood ashes ( soap + water
stearic acid + sodium hydroxide ( sodium stearate + water
C17H35COOH(s) + NaOH(aq) ( Na+1C17H35COO-1(aq) + H2O(l)
The Effect of Hard water on soap
2Na+1C17H35COO-1(aq) + CaCl2(aq) ( Ca(C17H35COO) 2(s) + 2NaCl(l)
Lost soap
Bath tub Scum
11) Water of hydration
CuSO4.5H2O copper(II) sulfate pentahydrate
CoCl2. 6H2O cobalt(II) chloride hexahydrate
Hygroscopic – gains H2O from atmosphere
Deliquescent - gains H2O from atmosphere & turns to a liquid-like solution
Efflorescent – loses H2O to atmosphere
Dessicant (Drying Agent)- used to keep chemicals dry in a dessicator
12) Acid-Base reactions
“ Neutralization reactions”
“Double Replacement Reactions”
Acid + base ( salt + water
HCl(aq) + NaOH(aq) ( NaCl(aq) + HOH(aq)
NaCl is the Salt of the Base – NaOH
NaCl is the Salt of the Acid – HCl
and Ba3(PO4)2 is the salt of the Base-Ba(OH)2 and the acid-H3PO4
Primary Standard- 1) Usually solid
2) High molecular mass
3) Stable at 100oC
4) High purity
Indicator- Phenolphthalein Acid/colorless
Neutral/colorless
Base/pink
Indicators tell when the titration is over
13) Buffers – resist changes in pH (see pH/pOH calculations)
a) Sodium bicarbonate neutralizes an acid
NaHCO3 + HCl ( NaCl + H2CO3
( H2CO3 ( H2O + CO2)
b) Sodium bicarbonate neutralizes a base
NaHCO3 + NaOH ( Na2CO3 + H2O
In both cases the sodium bicarbonate either removes H+1 or OH-1
from the solution. This is how a buffer works. Blood is a very complex
buffer system with a pH of about 7.4 The primary buffer is a mix of
H2CO3 (H2O(l) and CO2(g) ) and HCO3-1.
Stoichiometry
a) Mass-Mass Problems
1) Balance the reaction
2) Calculate the molecular mass of the known and the unknown
3) Calculate the number of moles of known
4) Calculate the number of moles of unknown
5) Calculate the number of grams of unknown
Grams known ( moles known ( moles unknown ( grams unknown
MM of Known Balanced MM of unknown
Reaction
Example
Calculate the mass of nitrogen needed to make 34 grams of ammonia.
1) Balance the reaction:
N2 + 3H2 ( 2NH3
2) Calculate the molecular mass of
the known and the unknown:
known 1N@14.0 = 14.0 unknown 2N @ 14 = 28 g N2
3H @ 1.0 = 3.0 1 mole N2
17 g NH3
mole NH3
3) Calculate the number of moles of known:
(34 grams NH3)(1mole NH3/17 grams NH3) = 2 moles NH3
4) Calculate the number of moles of unknown:
(2 moles NH3) ( 1 mole N2 / 2 moles NH3) = 1 mole N2
5) Calculate the number of grams of unknown:
(1 mole N2)(28 grams N2/mole N2) = 28 grams N2
All Together
grams N2 = (34 grams NH3) (1mole NH3) ( 1 mole N2) (28 grams N2) = 28 grams N2
(17 grams NH3) (2 moles NH3) (1 mole N2)
b) Molarity = moles solute/ Liter solution
2.0 moles NaOH/ 1 Liter solution = 2.0 molar NaOH = 2.0 M NaOH
Calculate molarity (moles/Liter)
Convert: Liters ( moles ( grams
Grams ( moles ( Liters
c) Dilution
Conc1 x Vol1 = Conc2 X Vol2
d) Percent composition = (grams solute/grams solution) x 100
Convert grams solute (( grams solution
grams solute ( ( grams solvent
grams solvent ( ( grams solution
e) pH / pOH / [H+1] / [OH-1]
1) acid pH =-Log [H+1]
[H+1] is the concentration of
hydrogen ions in moles/Liter
2) base pOH =-Log [OH-1]
[OH-1] is the concentration of
hydroxide ions in moles/Liter
[pic]
3) Acid [H+1] = 10-pH
4) Base [OH-1] = 10-pOH
[pic]
5) acid/base pH + pOH = 14
[pic]
-----------------------
Triple Point
4.58 mm of mercury
0.0098 oC
Gas
Liquid
Solid
Critical Temperature = 647.6 K
Critical Pressure = 217.7 atm
Vapor Pressure
Temperature
Calculator work
Type 1: pH / (+/-) / inverse Log gives [H+1]
Type 2: inverse Log / (+/-) / pH / enter gives [H+1]
pH can be replaced with pOH for bases
Calculator work
Type 1: [H+1] / Log / (+/-) gives pH
Type 2: (+/-) / Log / [H+1] / enter gives pH
[H+1] can be replaced with [OH-1] for bases
pH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
pOH 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0
More Acidic
More Basic
Neutral
Strong Acid Weak Acid Weak Base Strong Base
HCl HC2H3O2 NH4OH NaOH
Stomach Acid Vinegar Ammonia Water Oven Cleaner
De-ionized water
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