Lecture 8 - Solutions Flashcards
True/False: water has the ability to dissolve a wide variety of substances
True
aqueous solution = homogeneous or heterogeneous mixture
homogeneous
7 types of solutions: gas/gas gas/liquid liquid/liquid liquid/solid solid/liquid solid/solid gas/solid
air (O, N, and other gases) soda pop (CO2 in H2O) vinegar (acetic acid in H2O) dental fillings (Hg in Ag) sea water (NaCl in H2O) brass (Zn in Cu) nitrogen in steel
the measure of how much solute will dissolve in a solvent
solubility
solutions that contain the max amount of solute for the given conditions - cannot dissolve additional state
saturated solutions
why does the temperature always need to be specified when describing a saturated solution
because the solubility depends on temperature and temperature must be specified because of the “temperature effect” on solubility
most solids become more soluble in aqueous solution with _____ temperature
increasing
gas solubility decreases with _____ temperature for aqueous solutions
increasing
solutions that contain less than the max amount of solute - can dissolve additional state
unsaturated solutions
if a substance does not dissolve in a solvent
insoluble
contain a small amount of solute relative to what could dissolve
dilute solutions
contain a large amount of solute relative to what could dissolve
concentrated solutions
all solutes that dissolve in water can be divided into two categories
electrolyte
nonelectrolyte
a substance that dissolves in water to give an electrically conducting solution
electrolyte
a substance that dissolves in water to give a solution that conducts electricity poorly
nonelectrolyte
when an ionic substance dissolves in water it _____ into its ions
dissociates
component present in the greatest amount
solvent
component present in the relatively smaller amount
solute
substance that dissolve in each other in all proportions
miscible
what are gases always miscible
because the intermolecular attractions in the gas phase are always weak
when a dissolved solute forms a solid
crystallization
when the rate of dissolution and crystallization are equal
equilibrium
4 concepts for understanding equilibrium:
equilibrium is
- time dependent
- dynamic
- reversible
- temperature dependent
3 factors affecting the rate of solution formation and establishment of equilibrium
- surface area
- agitation
- temperature
increasing the pressure will _____ the solubility of a gas in a solvent
increase
decreasing the pressure will _____ the solubility of a gas in a solvent
decrease
the amount of solute dissolved in a given amount of solvent or solution
concentration
concentration equation:
concentration = (amt. solute/amt. solution)
% mass (solute) =
(mass solute/total mass solution) x 100
the ratio of the volume of a solute to the volume of the solution, multiplied by 100
volume-volume percent
% mass-volume =
(mass solute (g)/volume solution (mL)) x 100
Dilution Equation
CsVs = CdVd
properties that depend only on the number of solute particles in a solution and not on the nature of the solute particles
colligative properties
4 colligative properties
- vapor pressure lowering
- boiling point elevation
- freezing point depression
- osmotic pressure
the pressure required to stop osmosis
osmotic pressure
one solution has a lower osmotic presure
hypotonic
the solution with higher osmotic pressure
hypertonic
a concentration unit used to compare the osmotic pressures of different solutions
osmolarity
have similar properties to solutions but they are not true solutions
colloids
are colloids heterogeneous or homogeneous
heterogeneous
the scattering of light by colloidal-size particles
tyndall effect
collectively, the particles suspended in a colloid
dispersed phase
substance containing the colloid particles
dispersing medium
caused by collisions between the suspended particles and the molecules of the dispersing medium
brownian movement
