Chemistry "the Science In Context" Chapter 5

Front 1

solution

Back 1

homogeneous mixture of two or more substances

Front 2

solvent

Back 2

has the greater number of moles and is generally considered the "vehicle" for the solute. Seen as less important (less note-worthy) than the solute.

Front 3

solute

Back 3

has fewer moles than the solvent and is normally the substance of interest. solutions are generally labeled with the solute.

Front 4

aqueous solution

Back 4

water is the solvent

Front 5

concentration

Back 5

ratio of solute to solvent (or to the entire solution).
uses molality and molarity for units

Front 6

molarity

Back 6

moles of solute/liters of solution = mmol solute/mL solution.
used in problems involving osmotic pressure and stochiometry.

Front 7

molality

Back 7

moles of solute/kg of solvent.
used in problems involving freezing point depression and boiling point elevation.

Front 8

electrolyte

Back 8

any compound that can be dissolved into ions when placed in a solution.

Front 9

strong electrolyte

Back 9

completely dissolves into ions

Front 10

weak electrolyte

Back 10

partially dissolves into ions

Front 11

non-electrolytes

Back 11

do not dissolve into ions
(ex. ethanol)

Front 12

osmosis

Back 12

when solvent passes through a semipermeable membrane to balance the solute on each side of the membrane

Front 13

semipermeable membrane

Back 13

allows only solvent passage through the membrane

Front 14

density of water

Back 14

1.00g/mL

Front 15

dilute solution

Back 15

contains less solute than a concentrated solution (well water)

Front 16

concentrated solution

Back 16

contains more solute than a dilute solution (sea-water)

Front 17

dilution

Back 17

when more solvent is added to a solution

Front 18

boiling point

Back 18

determined by amount of dissolved solute particles
the more solute dissolved, the higher the boiling point

Front 19

Freezing Point Depression

Back 19

when solute is added, the freezing point lowers

Front 20

redox reactions

Back 20

oxidation/reduction reactions

Front 21

oxidation

Back 21

when electrons are lost

Front 22

reduction

Back 22

when electrons are gained

Front 23

oxidation number (ON)

Back 23

Charge that an atom possesses
halogens- ON= -1
alkali metals- ON= +1
alkaline earth metals- ON= +2
H- ON= +1 (sometimes -1)
O- ON= -2 (sometimes -1 or -1/2)

Front 24

oxidizing agents

Back 24

electron acceptors, they get reduced in a redox reaction

Front 25

reducing agents

Back 25

electron donors, they get oxidized

Front 26

acid-base

Back 26

neutralization (also an example of chemical equilibrium)

Front 27

acid

Back 27

donate H+ to the solution
(ex. HCl, HNO(3)

Front 28

base

Back 28

accepts H+
(ex. NaOH, KOH, Ca(OH)(2))

Front 29

molecular equation

Back 29

chemical equation in which all reactants and products are written as molecules, when in reality, they are ions in water.

Front 30

Net Ionic Equation

Back 30

Chemical equation in which all soluble species are written in their aqueous ionic form

Front 31

Saturated Solution

Back 31

a solution with the maximum amount of solute for a given volume of solvent

Front 32

unsaturated solution

Back 32

a solution with less than the amount of solute per volume of solvent.

Front 33

supersaturated solution

Back 33

temporary condition in which the solution contains more than the saturated amount.