Unit 4 Review

Question 1

mass %

Answer 1

(mass of solute / mass of solution) x 100%

% (m/m)

Question 2

volume %

Answer 2

(volume of solute / volume of solution) x 100%

% (v/v)

Question 3

mass / volume %

Answer 3

(mass of solute / volume of solution) x 100%

% (m/v)

Question 4

solute

Answer 4

the substance that dissolves

Question 5

solvent

Answer 5

the major component of the solution

Question 6

parts per million

Answer 6

(mass of solute / mass of solution) x 10^6

Question 7

parts per billion

Answer 7

(mass of solute / mass of solution) x 10^9

Question 8

molarity

Answer 8

moles per liter

Question 9

M =

Answer 9

moles / V

moles solute / liter solution

Question 10

moles (molarity equation) =

Answer 10

MV

Question 11

(Mi) (Vi) =

Answer 11

(Mf) (Vf)

Question 12

preparing dilute solutions

Answer 12

1) add the desired amount of solute to a volumetric flask
2) partially fill the flask, and mix
3) dilute to the correct volume

Question 13

ionic compounds ___________ in water

Answer 13

dissociate

Question 14

ionic equation

Answer 14

shows dissociated ions as separate species

Question 15

molar concentration of each ion in a solution

Answer 15

coefficient x molarity

Question 16

three colligative properties

Answer 16

1) freezing point depression
2) boiling point elevation
3) osmotic pressure

Question 17

freezing point depression

Answer 17

increase solute concentration = lower freezing point

more moles = lower freezing point

Question 18

boiling point elevation

Answer 18

antifreeze raises boiling point and lowers freezing point

Question 19

osmotic pressure

Answer 19

water moves toward the more concentrated solution

Question 20

hypertonic

Answer 20

in solution of high solute concentration

Question 21

hypotonic

Answer 21

in solution of low solute concentration

Question 22

conversion factor between solution volume and moles

Answer 22

molarity

Question 23

chapter 11 volume questions

Answer 23

1) balanced equation
2) determine mole ratio
3) calculate moles of first solution
4) calculate moles of the second solution
5) calculate the volume of the second solution by (moles / Molarity)
6) convert the volume to mL

Question 24

acids Arrhenius definition

Answer 24

produce H+ ions in water

Question 25

bases Arrhenius definition

Answer 25

produce OH- ions in water

Question 26

acids Bronsted-Lowry definition

Answer 26

compounds that donate H+ ions

proton (H+) donor

Question 27

bases Bronsted-Lowry definition

Answer 27

compounds that accept H+ ions

proton (H+) acceptor

Question 28

strong acid

Answer 28

completely ionize in water
ex. HCl, HBr, HI, H2SO4

Question 29

weak acid

Answer 29

partially ionize in water
ex. HF + H2O <-> H3O + F

Question 30

a conjugate base is identical to the acid, but…

Answer 30

without the H+

Question 31

a conjugate acid is identical to the base, but with an…

Answer 31

extra H+

Question 32

acid + base =

Answer 32

water + salt

Question 33

reactions of acids with metals

Answer 33

most metal react with acid to produce metal cations and hydrogen gas

Question 34

nonmetal oxides often react with water to form…

Answer 34

acids

Question 35

[H+] [OH-] =

Answer 35

1x10^-14

Question 36

pH + pOH =

Answer 36

14

Question 37

pH =

Answer 37

-log [H+]

Question 38

pOH =

Answer 38

-log [OH-]

Question 39

atomic and mass numbers have to be _______ on both sides of the equation

Answer 39

the same

Question 40

three major types of radioactive decay

Answer 40

alpha, beta, gamma

Question 41

alpha decay

Answer 41

emission of a helium nucleus (add Helium on products side)

Question 42

beta decay

Answer 42

-converts a neutron into a proton and electron
-emission of an electron

Question 43

predicting the material remaining using half-lives

Answer 43

start -> divide by two -> divide previous number by two -> continue

Question 44

isotopes

Answer 44

have the same atomic numbers but different mass numbers