unit 8 - solutions Flashcards by Hima Binu

solution

A homogeneous mixture of two
or more substances

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solutions contain…

particles of one substance that are uniformly spread out in another substance
ex: C6H12O6 (aq)

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parts of a solution

solute and solvent

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solute

the substance being dissolved

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solvent

the substance that dissolves the solute

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solution types - aqueous

water is the solvent

ex: NaCl (aq)
solute (NaCl), solvent (water)

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solution types - non aqueous

water is not the solvent

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solution types - tincture

alcohol is the solvent

ex: tincture of iodine
contains solute (I2), solvent (alcohol)

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solution characteristics

1) Clear or transparent- colorless or colored

2) Particles:
a. Are evenly distributed
(Solutions are homogeneous)
b. Do not settle out on standing
(particles dissolved stay dissolved)
c. Can not be separated by filtration

3) Variable Composition- A solution is a type of mixture, not a pure substance (compound)

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solubility

the amount of a solute to dissolve in a certain amount of solvent

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soluble

materials with a high degree of solubility (a lot dissolves)

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insoluble

materials with a low degree of solubility (little dissolves)

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factors that affect solubility: TEMPERATURE (Table G)

1) TEMPERATURE: (Table G)
- As temp increases solids become more soluble
- As temp increases gases become less soluble in water

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factors that affect solubility: pressure

2) PRESSURE:
- Pressure has little or no affect on the solubility of solid or liquid solutes
- As pressure increases gases become more soluble in liquids

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factors that affect solubility: type of solvent/solute

3) Type of Solute/Type of Solvent:

“Like Dissolves Like”
Polar Solutes dissolve in Polar solvents
Non-Polar solute dissolve in non-polar solvents.
Ionic Substances dissolve in Polar
solvents (salts in water)

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rate of solute dissolving

how fast a solute dissolves depends on frequency of interactions between solute and solvent

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factors that affect rate of solute dissolving

1) temperature - greater KE = more interactions
2) stirring - more interactions
3) surface area - grinding and chopping solute into pieces increases surface exposure and more interaction with solvent

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double replacement reactions and table F

Double Replacement Reactions:
Two compounds that react and produce a precipitate. Precipitate is the INsoluble Product!
Ex: Silver Nitrate (aq) + Sodium Chloride (s)
: AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3(aq)

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three degrees of saturation

saturation solution
unsaturated solutions
supersaturated solution

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saturated solutions

solution which contains the maximum amount of solute that can dissolve in a given amount of solvent at a certain temp.

point is given on the curve

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unsaturated solutions

solution that contains less than the maximum amount of solute that can dissolve at a certain temperature in a given amount of solvent
- point given is below the curve

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supersaturated solution

Solution that contains more than the maximum amount of solute than can dissolve (unstable), at a
certain temperature in a certain amount of solvent
- point given is above the curve

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measuring concentration by percent

% By Mass = mass of solute/mass of solution x 100

% By Volume = volume of solute/volume of solution x 100

1 PPM

= .0001%

PPM

expresses concentration as the mass of the solute in given amount of solution PPM = mass solute/mass solution x 1,000,000

evaporation

molecules on the surface of a liquid gain enough KE to break from the liquid and enter the gas phase ex: water on the floor or open container evaporates

boiling

liquid turns to a gas at any point in the container (not just the surface)

vapor

another word for gas phase

vapor pressure

the pressure that gas particles exert due to collisions above surface of a liquid

vapor pressures varies directly with...

TEMPERATURE regardless of the volume

boiling point

Temperature at which the Vapor pressure is equal to Atmospheric Pressure *At standard pressure - Normal Boiling Point *low atmospheric pressure - above sea level *high atmospheric pressure- below sea level

normal boiling point

temperature at which the vapor pressure exerted by the liquid is equal to Standard Atmospheric Pressure 1 atm, 101.3 Kpa, 760 torr or mmHg

temperature and vapor pressure

as temperature increases so does the vapor pressure of a liquid

table H - remember boiling point

the temperature at which the vapor pressure equals 101.3 kPa

diluted solution

solution in which a small amount of solute in a given amount of water less solute, more water

concentrated solution

solution which a large amount of solute in a given amount of water more solute, less water

how do we build a solution

1) put salt in flask 2) add total amt of H2O needed in the problem

molarity

the concentration of a solution in moles of solute per liter of solution

to get L from mL

do mL/1000

as molarity increases, what happens to solution concentration

solution is more concentrated

how can we change the concentration (molarity) of a solution by perfoming a dilution

add water to change a higher concentration to a lower concentration

moles of a substance before dilution are ...

equal to the moles of a substance after dilution

steps to performing a dilution

1. find V1 2. fint amount of H2O to dilute (V2-V1 = amt of water) 3. put water into flask first, then add concentrated soution

colligative properties

when you take a pure substance, (ex. water), and add any other substance to it, you affect the original substance's boiling point and freezing point

concentration of dissolved particles impacts the

boiling point and freezing point of a substance

as concentration increases

the more moles of particles of the solute exist (remember we measure concentration in (M) molarity)

the greater the concentration or more solute particles, original substance will have its freezing and boiling point...

boiling point increased, freezing point decreased

no matter what is added to a substance, the response will always be the

SAME

colligative properties conclusions: boiling point...? why?

increases It takes a higher temp (greater Kinetic Energy) for the appropriate collisions to occur between the gas particles in order to break intermolecular bonds

colligative properties conclusions: freezing point...? why?

decreases It takes a lower temp (lower KE) for all the liquid particles to come together to form intermolecular bonds and become a solid.

do ionic substances dissociate into +/- ions?

YES

do covalent substances (molecules) dissociate into +/- ions?

which will always produce more moles of particles compared to the other

IONIC substances will always produce MORE moles of particles compared to COVALENT substances Ex. 1 Mole NaCl → 1 mol Na+ + 1 mol Cl- (total is 2 mol of particles) Ex. 1 Mole C6H12O6 → 1 mol C6H12O6

the higher the boiling point, the ____ the substances vapor pressure

lower

the lower the boiling point, the _____ the substances vapor pressure

higher