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SolutionsChemistry
Mrs. Nunez
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Solution - homogeneous mixture
Solvent - present in greater amount
Solute - substance being dissolved
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Solvation the process of dissolving
solute particles are separated and pulled into solution
solute particles are surrounded by solvent particles
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StrongElectrolyte
Non-Electrolyte
solute exists asions only
- +
salt
- +
sugar
solute exists asmolecules only
- +
acetic acid
WeakElectrolyte
solute exists asions andmolecules DISSOCIATION IONIZATION
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Dissociationseparation of an ionic solid into aqueous ions
NaCl(s) Na+(aq) + Cl–(aq)
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Ionization breaking apart of some polar molecules into aqueous ions
HNO3(aq) + H2O(l) H3O+(aq) + NO3–(aq)
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Molecular Solvation
molecules stay intact
C6H12O6(s) C6H12O6(aq)
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NONPOLAR
NONPOLARPOLARPOLAR
“Like Dissolves Like”
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C. Johannesson
Soap/Detergentpolar “head” with long nonpolar “tail”dissolves nonpolar grease in polar water
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SolubilitySATURATED SOLUTIONno more solute dissolves
UNSATURATED SOLUTIONmore solute dissolves
SUPERSATURATED SOLUTIONbecomes unstable, crystals form
concentration
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Solubilitymaximum grams of solute that will
dissolve in 100 g of solvent at a given temperaturevaries with tempbased on a saturated soln
Factors determining rate of solution...1. stirring (agitation)2. surface area the dissolving particles3. temperature
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C. Johannesson
C. SolubilitySolids are more soluble at...
high temperatures.
Gases are more soluble at...• low temperatures &• high pressures
(Henry’s Law).• EX: nitrogen narcosis,
the “bends,” soda
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SolubilitySolubility Curveshows the dependence of solubility on temperature
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Solids tend to dissolve best when:•They are heated
•They are stirred•Crushed into smaller particles
Gases tend to dissolve best when:
•The solution is cold•The pressure is high
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LiquidsMiscible means that two liquids can dissolve in each otherwater and antifreezewater and ethanol
Partially miscible- slightlywater and ether
Immiscible means they can’toil and vinegar
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Gases in liquids...Henry’s Law - says the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquidthink of a bottle of soda pop, removing the lid releases pressure
Equation: S1 S2 P1 P2
Sample 16.1, page 477
=
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ConcentrationThe amount of solute in a solution.Describing Concentration
% by mass - medicated creams% by volume - rubbing alcoholppm, ppb - water contaminantsmolarity - used by chemistsmolality - used by chemists
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Concentrated vs. Dilute
Lots of solute, in a
small amount of solvent.
Small amount of solute in a
large amount of solvent.
Notice how dark
the solutions appears.
Notice how
light the solution appears.
CONCENTRATED
DILUTE
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A. MolarityConcentration of a solution.
solution of literssolute of moles(M)Molarity
total combined volume
substance being dissolved
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Molarity
2M HCl
LmolM
L 1HCl mol 2HCl 2M
What does this mean?
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Molarity CalculationsFind the molarity of a 250 mL solution containing 10.0 g of NaF. 10.0 g 1 mol
41.99 g = 0.238 mol NaF
0.238 mol0.25 L
M = = 0.95M NaF
LmolM
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B. Molality
solvent ofkg solute of moles(m)molality
mass of solvent only
1 kg water = 1 L waterkg 1mol0.25 0.25m
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MolalityFind the molality of a solution containing
75 g of MgCl2 in 250 mL of water.
75 g MgCl2 1 mol MgCl2
95.21 g MgCl2
= 3.2m MgCl2
0.25 kg water
kgmolm
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2211 VMVM
C. DilutionPreparation of a desired solution by adding water to a concentrate.
Moles of solute remain the same.
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DilutionWhat volume of 15.8M HNO3 is required to make 250 mL of a 6.0M solution?
GIVEN:M1 = 15.8MV1 = ?M2 = 6.0MV2 = 250 mL
WORK:M1 V1 = M2 V2
(15.8M) V1 = (6.0M)(250mL)
V1 = 95 mL of 15.8M HNO3
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Preparing Solutions500 mL of 1.54M
NaCl
500 mLwater
45.0 gNaCl
• mass 45.0 g of NaCl• add water until total
volume is 500 mL• mass 45.0 g of NaCl• add 0.500 kg of water
500 mLmark
500 mLvolumetricflask
1.54m NaCl in 0.500 kg of water
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Preparing Solutions250 mL of 6.0M HNO3
by dilutionmeasure 95 mL
of 15.8M HNO3
95 mL of15.8M HNO3
water for safety
250 mL mark
• combine with water until total volume is 250 mL
• Safety: “Do as you oughtta, add the acid to the watta!”
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Percent solutions can be expressed by a) volume or b) mass
Percent means parts per 100, so
Percent by volume: = Volume of solute
x 100% Volume of solution
indicated %(v/v)Sample Problem 16.5, page 485
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Percent solutions
Another way to do mass percentage is as mass/mass:
Percent by mass: = Mass of solute(g)
x 100% Mass of solution (g)
Indicated %(m/m)
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property that depends on the concentration of solute particles, not their identity
Colligative Property
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TypesFreezing Point Depression (tf)
f.p. of a solution is lower than f.p. of the pure solvent
Boiling Point Elevation (tb)
b.p. of a solution is higher than b.p. of the pure solvent
Vapor pressure lowering
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- Page 488
Glucose will only have one particle in solution for each one particle it starts with.
NaCl will have two particles in solution for each one particle it starts with.
CaCl2 will have three particles in solution for each one particle it starts with.
Colligative Properties
Some particles in solution will IONIZE (or split), while others may not.
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Freezing Point Depression
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Solute particles weaken IMF in the solvent.
Boiling Point Elevation
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- Page 494The addition of a solute would allow a LONGER temperature range, since freezing point is lowered and boiling point is elevated.
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Applicationssalting icy roadsmaking ice creamantifreeze
cars (-64°C to 136°C)