chapter 4

Question 1

solute

Answer 1

substance being dissolved

Question 2

solvent

Answer 2

usually H2O, does the dissolving

Question 3

electrolyte

Answer 3

substance that, when dissolved in water, is able to produce a solution that conducts an electrical charge

Question 4

solvation

Answer 4

process where solid is pulled into the solution, will be clear if fully solvated.

Question 5

suspension

Answer 5

mixture of solid and liquid where liquid doesn’t dissolve solid

Question 6

strong electrolyte

Answer 6

conduct current very well, completely ionized in water. from ionic compounds and strong acids/bases.

Question 7

weak electrolyte

Answer 7

conducts small current, small ionization

Question 8

non-electrolyte

Answer 8

no current. dissolves in water but does not form ions

Question 9

what are the strong electrolytes?

Answer 9

acids, bases, salts

Question 10

strong acids (5)

Answer 10

HCl, HBr, HI, HNO3, H2SO4

Question 11

strong bases (4)

Answer 11

NaOH, KOH, LiOH, Ca(OH)2

Question 12

salts (3)

Answer 12

NaCl, KBr, MgCl2

Question 13

weak acids (3)

Answer 13

HF, HC2H3O2, H2CO3

Question 14

weak base

Answer 14

NH3

Question 15

molarity

Answer 15

moles of solute per volume of solution in a liter

Question 16

dilution

Answer 16

the process of adding water to decrease the concentration of a solution, doesn’t change mol quantity of solute

Question 17

dilution formula

Answer 17

(initial molarity)(initial volume) = (final molarity)(final volume)

Question 18

if we know the concentration of a solution, it’s called a

Answer 18

standard solution

Question 19

stock solution

Answer 19

standard solution you can stockpile

Question 20

moles formula

Answer 20

molarity x liters

Question 21

3 reactions in aqueous solutions

Answer 21

precipitation, acid-base, oxidation-reduction

Question 22

precipitation reaction

Answer 22

double displacement reaction in which a solid forms and separates (precipitate)

Question 23

spectator ions

Answer 23

do nothing in precipitate reaction

Question 24

solubility rules

Answer 24

1. most NO3- are soluble
2. most alkali metals (group a1), salts, and NH4+ salts are soluble
3. most halogens are soluble except silver, lead, and mercury
4. oxygenated halogen ions are soluble
5. most sulfate salts are soluble (except BaSO4, PbSO4, HgSO4, and CaSO4)

Question 25

a salt is a ... pairing

Answer 25

cation, anion

Question 26

molecular equation

Answer 26

overall balanced chemical equation

Question 27

complete ionic equation

Answer 27

all soluble species as ions, balanced

Question 28

net ionic equation

Answer 28

only represents ions that equal solids

Question 29

types of acid-base reactions

Answer 29

arrhenius, bronsted-lowry, lewis

Question 30

Arrhenius definition

Answer 30

Acid is the proton (H+) donor; base is the OH- donor

Question 31

Bronsted-Lowry definition

Answer 31

acid is the proton donor, base is the proton acceptor

Question 32

lewis

Answer 32

Acid is the electron pair acceptor, bae is the electron pair donor

Question 33

neutralization

Answer 33

process of allowing an acid and a base to react together so that there are fewer, if any, acidic or base ions left

Question 34

titration

Answer 34

delivery of a measured volume of a solution of known concentration (titrant) into a solution of an unknown concentration of a substance being analyzed (analyte)

Question 35

equivalence point

Answer 35

enough titrant is added to react exactly with the analyte

Question 36

end point

Answer 36

point at which a usual indication, caused by the indicator, shows that the equivalence point has passed

Question 37

oxidation-reduction reactions

Answer 37

1 or more electrons are transferred

Question 38

oxidation state

Answer 38

a # assigned to an atom that describes the degree of oxidation or loss of e-

Question 39

if an atom loses e-

Answer 39

oxidized

Question 40

if an atom gains e-

Answer 40

reduced

Question 41

covalent molecules share electrons, so...

Answer 41

they do not have full + or - charges

Question 42

oxidation numbers show...

Answer 42

a fictional charge

Question 43

oxidation state rules

Answer 43

1. The oxidation state of an atom in an elemental state is 0 2. Oxidation state of a monoatomic ion = the charge of the ion 3. Oxygen = -2 in covalent compounds except peroxides where it is -1 4. hydrogen = +1 5. Fluorine = -1 6. sum of oxidation state must equal 0 in compounds 7. sum of oxidation states = the charge of the ion, if ionic

Question 44

a compound that is oxidized is called...

Answer 44

the reducing agent

Question 45

a compound that is reduced is called...

Answer 45

the oxidizing agent

Question 46

redox rules

Answer 46

1. write unbalanced 2. determine oxidation states 3. show gain or loss of e- 4. use coefficients to equalize electron flow 5. balance the rest by inspection