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37 Cards in this Set

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how are the solute particles distributed in a solvent
evenly
the effect of temperature on solubility
solutbility increases with an increase in temp of solution
growing of crystals takes andvantage of the decreasing solutibity with decreasing temp
solutibily of dissolved gas decreases as the temp increases
liquid-liquid solution
vinegar
(acetic acid in h20)
cleaning solutions
suspensions
large particles in a solvent will settle out
example-muddy water
salad dressings
solvation process
1. crystal is pounded by h2o molecules
2. na plus and cl minus ions are removed
3. ions become surrounded by h2o creating solution
tyndall effect
occurs when light is scatered by colloidal particles dispersed in a transparent medium.
a propoerty that can be used to distinguish between a solution and a colloid
rate of dissolution
increases with increase in surface area
solution equilibrium
the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates
unsaturated solution
a solution that contains less solute than a saturated solution under the existing conditions
concentration
a measure of the amount of solute in a given amount of solvent or solution
solution
any substance that is evenly dispersed or distributed throughout another substance
immiscible liquids
two liquids that dont mix
give an example of a gas liquid solution
humidity in air
co2 in soda
solid-liquid solution
sea water
(all elements dissolved in h20)
heterogeneous mixtures
oil and water
mixtures of different things
dissociation equation
nacl- na plus and cl minus
hydration
the solution process with water as the solvent
dissociation
process of decomposition of a crystal into hydrated ions
unsaturated solution
a solution that is able to dissolve more solute
effect of pressure on solubility
if a carbonated drink is opened bubles rise to the liquids surface and are released but it can be stopped if the cap is refrigerated
solubility of gas depends on the pressure acting upon the system
suspension paticles
are 1000 times larger than atoms or molecules
electrolytes
a substance which will conduct electricity when dissoved in h20
h3o
hydronium ion
solubility
is the amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature
saturated solution
a solution that contains the maximum amount of dissolved solute
molarity
number of moles of solute in one liter of solution
molarity= amount of solute (mol)/ volume of solution (L)
colligative properties
properties that depend on the concentration of solute particles but not on their identity
polar-polar solvent/solute combination
solvation occurs b/c of the attraction between the two and the solute molecules disperse throughout solution
misceible liquids
when there is no apparent to the solubility of one substance in another
solubility
the amount of substance needed to make a saturated solution at a specified temperature
the atmosphere as a solution
nitrogen is the solvent
co2 o2 h2 are all solutes
it is a gas gas solution
colloids
particles intermediate in size between solutions and suspensions. cooloids remain suspended due to particle motion
example- milk, mayonnaise
couds, fog
nonelectrolytes
a substance will not conduct when dissolved
example-sugars c6h12o6
supersaturated solution
a solution that contains more dissolved solute than a saturated solution conatins under the same conditions
henry's law
the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
nonpolar- nonpolar solvent/solute combination
will not disoolve in water composed of polar molecules
saturated solution
a solution that cannot disolve any more solute at a given temperature