chapter 8

Question 1

define solution

Answer 1

a homogeneous mixture of two or more substances

Question 2

define solvent and solute

Answer 2

solvent- substance present in the largest quantity (only 1)
solute- substance(s) present in lesser quantity

Question 3

define aqueous solution

Answer 3

where water is the solvent

Question 4

define concentration

Answer 4

amount of solute dissolved in a given amount of solvent or solution

Question 5

define net ionic equation

Answer 5

shows only the atoms/molecules involved in the rxn

Question 6

define full ionic equation

Answer 6

shows whats happening in solution

Question 7

define molecular (chemical) equation

Answer 7

a shorthand. not separated out

Question 8

define solubility

Answer 8

how much of a particular solute can dissolve in a given volume of solution.

Question 9

define saturated

Answer 9

maximum amount of solute dissolved (per volume) at a given temperature/pressure

Question 10

define unsaturated

Answer 10

sub-maximum amount of a solute dissolved(per volume)at a given temperature/pressure

Question 11

define supersaturated

Answer 11

over maximum but stays soluble until precipitation is seeded

Question 12

describe molarity( part of concentration)

Answer 12

moles solute/liters of solution (mol/L). “molar solution” ex: 125g NaCl in 2.5L of solution. g NaCl divided by molar mass. get answer divide by liters and get answer. this says for every 1L there is x mols

Question 13

ex of M concentration: “how many moles of NaOH are in 10.0 mL of a 5.0M NaOH solution?”

Answer 13

(10mL)(1L/1000mL)(5.0 mol/1L)=0.050 moles

Question 14

ex of M concentration: “how many liters do you need to make a 0.2 M NaOH solution with 2.2 g NaOH?”

Answer 14

(2.2 g NaOH)(1 mol/40.00 g NaOH)(1L/0.2 mol)=0.275 L

Question 15

formula for molarity and dilutions

Answer 15

mol/L
(M1)(V1) —–> (M2)(V2)
stock. working
concentration concentration

Question 16

how to tell if its a molarity dilution problem?

Answer 16

first M given is more than what you want out of it
will say “by diluting’

Question 17

set up formula: “make 50 mL of a 0.05 M working solution from a 2.0 M stock solution of___”

Answer 17

(2.0M)(V1)/(0.05M)(0.05L)

Question 18

define electrolyte and example:

Answer 18

ions in a solution, formed from solutes that dissociate into ions. (carry an electric current).
H2O
ex: NaCl(s) —–> Na+(aq) + Cl-(aq
1 mol. 2 mol
ONLY IONIC COMPOUND BREAK DOWN

Question 19

define nonelectrolyte and example:

Answer 19

no ions in solution, dissolves but doesnt dissociate. (stays covalently bonded molecule)
H2O
glucose(s) ——–> glucose (aq)
1 mol. 1 mol

Question 20

define strong electrolyte

Answer 20

dissociates virtually 100%
ex” NaCl thing

Question 21

define weak electrolyte

Answer 21

only partially dissociates
ex: CH3COOH(aq) <====> H+(aq) + CH3COO-
EQUILIBRIUM

Question 22

define acid and ex

Answer 22

donates H+ to solution(in water)
ex: HCl(aq) —> H+(aq) + Cl-(aq)

Question 23

define base and ex

Answer 23

accepts H+ from solution(inH2O)
ex: NH3(aq) +H2O –> NH4+ + OH-(aq)
water acts as acid

Question 24

whats acids and bases theory called

Answer 24

brønsted-lowry theory

Question 25

describe hydronium ion when acid and bases

Answer 25

H+ in solution are combined with H2O to form H3O+
ex: from acid- H+(aq) + H2O(l) —> H3O+ (aq)

Question 26

describe hydrochloric acid base process

Answer 26

H2O(l) + HCl(aq) —> Cl-(aq) + H3O+(aq)
WATER ACTS AS BASE

Question 27

define amphoteric

Answer 27

can behave as acid and base (WATER) (H2CO3)

Question 28

define monoprotic acids and diprotic acids and how

Answer 28

mono- loses 1H+
di- loses 2 H+
poly exists.
DI AND POLY GO THRPUGH RXN MULTIPLE TIMES TILL H IS OUT

Question 29

what is the heart of all acid/base chemistry

Answer 29

H+(aq) + OH-(aq) —> H2O(l)

Question 30

how to solve neutralization rxn: “you spill 20.0 mL of 3.5 M HCl in lab. what volume of 5M NaOH is required to neutralize the acid?”

Answer 30

set up ionic equation and get net(H+ + OH- —> H2O(l) ). use spill given(20mL) convert to L multiple by (3.5 mol HCl/1L) then do molar ratio from net (1 molH+/ 1mol HCl) and get 0.07 mol H+
take that answer as given then do molar ratio pf net (1 mol OH-/ 1 mop H+) then do another molar ratio ( 1 mol NaOH/ 1 mol OH-) and then do (1L/ 5 mol NaOH) and get 0.014 L 5M NaOH or 14 mL

Question 31

define oxidation

Answer 31

lose of electrons
gain O lose H

Question 32

define reduction

Answer 32

gain of electrons
lose O gain H

Question 33

ex of redox reaction (reduction and oxidation happen simultaneously)

Answer 33

ANY ELEMENT YOU FIND IN NATURE = zero neutral
Mg°(s) + Cl°2(g)—>Mg²+(aq) + 2Cl-(aq)
Mg lost 2e-(ox) Cl gain 2e-(re)
break into 1/2 rxns.
Mg: Mg°(s)—> Mg²+(aq) + 2e-
Cl: Cl°2(g) + 2e- —> 2Cl-(aq)

Question 34

do 1/2 redox rxns where you have to multiple so e- are same : Al°(s)+ O°2(g) –> Al2O3(s)

Answer 34

ox1/2:(Al°—>Al3+ +3e-) x 4
red1/2:(O°2+ 4e- –> 2O2-) x3
4Al°(s)—>4Al3+(aq) + 12e-
3O°2 + 12e- –> 6O(2-)(aq)
4Al°(s) + 3O°2 –> 4Al(3+) +6O(2-)
2Al2O0