Exam 2

Question 1

solution

Answer 1

a homogenous mixture made up of a solute and solvent

Question 2

solvent

Answer 2

generally present in larger amounts and does not change shape (ex: salt water) - what is doing the dissolving

Question 3

solute

Answer 3

present in smaller amounts and might change shape (ex salt) - what is being dissolved

Question 4

aqueous solution

Answer 4

water is solvent and used to dissolve the solution

Question 5

concentration

Answer 5

general term referring to relative amounts of solute and solvent

Question 6

dilute

Answer 6

relatively small amounts of solute

Question 7

molarity formula

Answer 7

of moles in solute/ #liters of water

Question 8

chemical reaction types

Answer 8

1. Precipitation reactions - exchange of ions (switch metals)
2. acid-base reaction - transfer of a proton (H+)
3. oxidation-reduction reactions - transfer of electrons

Question 9

precipitate reaction table

Answer 9

Compound of
Li+, Na+, K+, NH4+, NO3-, CH3OO-, HCO3-, ClO3- —-> ALWAYS SOLUABLE

Cl-, Br, I- —-> insoluble with Ag+, Ag2+, Pb2+

F- —-> insoluble with Pb2+, Fe3+

SO4(-2) —-> insoluble with Ag+,Ag2(2+), Pb2+, Ba2+, Sr+

CO3(_2), PO4(-3), CrO4(-2), S(-2) —-> soluble with Li+, Na+, K+, and NH4+

HO- —> soluble with Li+, Na+, K+, NH4+ (group 1) and Ba(2+)

Question 10

strong acid

Answer 10

completely ionizes (breaks apart) in water

Question 11

weak acid

Answer 11

partially breaks apart in water

Question 12

strong base

Answer 12

completely breaks apart in water to give an HO-

Question 13

weak base

Answer 13

partially breaks apart in water to give an HO-

Question 14

strong acids (7)

Answer 14

HCl - hydrochloric acid
HNO3 - nitric acid
H2SO4 - Sulfuric Acid
HBr - hydrobromic acid
HI - hydroiodic acid
HClO4 -perchloric acid
HClO3 - chloric acid

Question 15

Weak Acids (7)

Answer 15

HO2C2O2H - Oxalic acid
H2SO3 - Sulfurous acid
H3PO4 - Phosphoric acid
HNO2 - Nitrous acid
C6H5COOH - Benzoic acid
CH3COOH - Acetic acid
HCOOH - Formic acid

Question 16

Oxidation

Answer 16

loss of electrons (but getting higher in numbers)

Question 17

reduction

Answer 17

gain of electrons (getting lower in numbers)

Question 18

rules for oxidation numbers

Answer 18

1. If element is alone then its 0
2. if there’s a charge when its alone its that charge
3. oxygen is -2 except in peroxide (O2(-2) its -1)
4. hydrogen is 1+ w/ most nonmetals and -1 with metals
5. fluorine is always -1 in its compounds
6. the sum of oxidation numbers of all atoms must equal the charge on the species (zero for neutral species)

Question 19

balancing- oxidation-reduction equations rules

Answer 19

1. write 2 half reactions
2. figure out oxidation numbers and oxidation/reductions
3. Balance oxygen by adding H2O molecules
4. Blanca hydrogen atoms by adding H+ ions
5. balance the charge by adding electrons
6. if needed multiply each half-reaction by the smallest possible integer
7. add the half-reactions together and simplify by removing species that appear on both sides of equations

Question 20

if an equation is under basic conditions

Answer 20

Proton cannot exist any H+ so add an OH-

Question 21

concentration solving

Answer 21

when volume goes up concentration goes down and vice versa (mxv = your concentration)

if your give the same compound twice then find a concentration of each then divide by the final volume (m1v2+m2v2/v3)