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Mixture
Combination of 2 or more kinds of matter, where each retains its own composition and properties
Homogeneous
Mixture with uniform composition (like salt water)
Heterogeneous
Mixture without uniform composition (like dirty water)
Solution
A homogeneous mixture in a single phase
Properties of solutions
uniform distribution of particles
will not settle out
transparent
can’t be filtered out (small particle size)
solute
the part that gets dissolved (typically lesser amount)
solvent
the part that does the dissolving (typically the greater amount)
Aqueous (aq)
solution that contains water as the solvent
Tinctures
solutions that contain alcohol as the solvent
Electrolyte
Anything that dissolves in water and conducts electricity (charged ions)
Suspensions
Heterogeneous mixture of the largest particles that do settle out (muddy water, pepto bismol, antacids)
Colloids
Contain intermediate size particles that remain in suspension because the DO NOT settle out (mayonnaise, foam, smoke, fog)
Degree of solubility
The amount of substance required to form a saturated solution in a certain amount of solvent at a certain temperature
3 ways to help dissolving occur
Crushing, stirring, heating
Ionic subtances dissolve in polar substances
salt in water
nonpolar substances dissolve in nonpolar substances
oil and gasoline
Immiscible substances
do not dissolve in each other (oil and vinegar in salad dressing)
Miscible substances
do not dissolve in each other in any proportion (alcohol and water)
For solids-Solubility increases as
temperature increases
For gases- solubility decreases as
temperature increases
gases only- as pressure increases
solubility increases
Henry’s law
solubility is proportional to pressure
Effervescence
the escape of a gas from a solution (like a soda bottle)
Steps for Solubility and energy changes when creating a solution
Breakup the solute (endothermic)
Breakup the solvent (Endothermic)
Formation of the solution (exothermic)
Heat of solution
the amt of heat absorbed or released when a solute dissolves in a solvent (heat of steps 1, 2, 3)
Heat of hydration
energy released when ions are surrounded by water molecules (heat of only step 3)
As the size of the ion decreases…
increased heat released
As the charge of the ion increases…
increased heat released
Dissociation
separation of ions caused by the action of the solvent (process of steps 1 and 2)
Hydration
The process of the solute particles being surrounded by water molecules (process of step 3)
O2 and CO2 are __________ so they…
nonpolar, dont dissolve much in water
soluble
more than one gram of solute dissolves per 100g of water
slightly soluble
between 0.1 and 1 g dissolves
insoluble
less than 0.1 g dissolves
Saturated
the solution dissolves as much solute as it can at a given temperature and a certain amount of solvent
unsaturated
the solution is currently dissolving less than the maximum amount of solute that can be dissolved at a given temperature
saturated with undissolved particles
the solution dissolves as much solute as it can at a given temperature and certain amount of solvent AND some particles are undissolved at the bottom of the container
supersaturated
the solution currently holds more than the maximum amount of solute at a given temperature (ex- sodium acetate and sodium thiosulfate)
In a solubility graph, points on the line are
saturated
In a solubility graph, points under the line are
unsaturated
In a solubility graph, points above the line are
saturated with undissolved particles
dilute
a small amount of solute in a large amount of solvent
concentrated
a larger amount of solute in a smaller amount of solvent
% solute in a solution general formula and three types
%=(solute/solution)100 OR %=(solute/solute + solvent) 100
weight/weight (chem industry)
weight/volume (medical IV)
volume/volume (alcohol solutions)
Molarity formula and what is it used for
M= moles solute/ liters of solution
used to calculate concentration
Molality formula and what its used for
m= moles solute/ kg of solvent
used to calculate concentration
Dilution Formulas (two of them)
CoVo = CnVn OR MoVo=MnVn
C=concentration
M= MOLARITY
What dissociates?
ionic compounds, and acids ionize (dissociation of a covalent compound)
What substances do not dissociate
Substances that are not acids, bases, or salts
When solutes dissolve in liquids…
they lower the freezing point
What two factors affect the degree of change in temp?
amount of solute and nature of the solvent
Colligative properties
A property that depends on the concentration (ex- freezing and boiling point)
freezing point formula
change in Tf= kf(m)(x) in water, kf=- 1.86 degrees m= molality |
as the number of solute particles increases…
the freezing point decreases
boiling point formula
change in Tb= Kb(m)(x) in water,Kb= 0.512 degrees m= molality |
more solute= ______ vapor pressure
less
Note
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