Chemistry

Front 1

how are the solute particles distributed in a solvent

Back 1

evenly

Front 2

the effect of temperature on solubility

Back 2

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

Front 3

liquid-liquid solution

Back 3

vinegar
(acetic acid in h20)
cleaning solutions

Front 4

suspensions

Back 4

large particles in a solvent will settle out
example-muddy water
salad dressings

Front 5

solvation process

Back 5

1. crystal is pounded by h2o molecules
2. na plus and cl minus ions are removed
3. ions become surrounded by h2o creating solution

Front 6

tyndall effect

Back 6

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

Front 7

rate of dissolution

Back 7

increases with increase in surface area

Front 8

solution equilibrium

Back 8

the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates

Front 9

unsaturated solution

Back 9

a solution that contains less solute than a saturated solution under the existing conditions

Front 10

concentration

Back 10

a measure of the amount of solute in a given amount of solvent or solution

Front 11

solution

Back 11

any substance that is evenly dispersed or distributed throughout another substance

Front 12

immiscible liquids

Back 12

two liquids that dont mix

Front 13

give an example of a gas liquid solution

Back 13

humidity in air
co2 in soda

Front 14

solid-liquid solution

Back 14

sea water
(all elements dissolved in h20)

Front 15

heterogeneous mixtures

Back 15

oil and water
mixtures of different things

Front 16

dissociation equation

Back 16

nacl- na plus and cl minus

Front 17

hydration

Back 17

the solution process with water as the solvent

Front 18

dissociation

Back 18

process of decomposition of a crystal into hydrated ions

Front 19

unsaturated solution

Back 19

a solution that is able to dissolve more solute

Front 20

effect of pressure on solubility

Back 20

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

Front 21

suspension paticles

Back 21

are 1000 times larger than atoms or molecules

Front 22

electrolytes

Back 22

a substance which will conduct electricity when dissoved in h20

Front 23

h3o

Back 23

hydronium ion

Front 24

solubility

Back 24

is the amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature

Front 25

saturated solution

Back 25

a solution that contains the maximum amount of dissolved solute

Front 26

molarity

Back 26

number of moles of solute in one liter of solution
molarity= amount of solute (mol)/ volume of solution (L)

Front 27

colligative properties

Back 27

properties that depend on the concentration of solute particles but not on their identity

Front 28

polar-polar solvent/solute combination

Back 28

solvation occurs b/c of the attraction between the two and the solute molecules disperse throughout solution

Front 29

misceible liquids

Back 29

when there is no apparent to the solubility of one substance in another

Front 30

solubility

Back 30

the amount of substance needed to make a saturated solution at a specified temperature

Front 31

the atmosphere as a solution

Back 31

nitrogen is the solvent
co2 o2 h2 are all solutes
it is a gas gas solution

Front 32

colloids

Back 32

particles intermediate in size between solutions and suspensions. cooloids remain suspended due to particle motion
example- milk, mayonnaise
couds, fog

Front 33

nonelectrolytes

Back 33

a substance will not conduct when dissolved
example-sugars c6h12o6

Front 34

supersaturated solution

Back 34

a solution that contains more dissolved solute than a saturated solution conatins under the same conditions

Front 35

henry's law

Back 35

the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

Front 36

nonpolar- nonpolar solvent/solute combination

Back 36

will not disoolve in water composed of polar molecules

Front 37

saturated solution

Back 37

a solution that cannot disolve any more solute at a given temperature