Chapter 9 General Properties of Aqueous solutions

Question 1

solution

Answer 1

a homogenous mixture

Question 2

solute

Answer 2

the analyze of interest

Question 3

solvent

Answer 3

the medium in which the solute is dissolved or dispersed

Question 4

Aqueous solutions

Answer 4

a solution in which the water is the solvent

Question 5

solubility

Answer 5

the maximum amount of substance that will dissolve into a solvent at a given temperature

Question 6

saturated solution

Answer 6

a solution that contains the maximum amount of dissolve solid

Question 7

electrolytes vs. non-electrolytes

Answer 7

once dissolved, different substances may behave differently and results in different types of solutions

Question 8

electrolyte

Answer 8

substance that dissolve in water to form solutions that conduct electricity

Question 9

non-electrolytes

Answer 9

substances that dissolve in water to form solutions that do not conduct electricity

Question 10

electrolytes form ions there are two ways ion can be formed:

Answer 10

Dissociate: to separate, upon dissolving to form separate ions

ionize:the process in which a. molecular compound formed an ion

Question 11

strong electrolytes

Answer 11

substances that dissociate or ionize completely

soluble salts, strong acids, strong bases

Question 12

weak electrolytes

Answer 12

substances that partially dissociate or ionize

slightly soluble slats, weak acids, weak bases

Question 13

conductivity

Answer 13

non-electrolytes: no ions-does not conduct electricity

molecular compounds(not acid/base)

strong electrolyte: lots of ions-conducts electricity very well

soluble salts

Question 14

Soluble

Answer 14

1. compounds containing an alkali metal cation(Li+,Na+,K+,Rb+,Cs+) or the ammonium ion(NH4+)
2. compounds containing the nitrate ion(NO3-), acetate ion(C2H3O2-) or chlorate ion(ClO3-)
3. compounds containing the chloride ion (Cl-), bromide ion(Br-), or iodide ion(I-)
   exceptions: compound that contains Ag+,Hg2^2+,Pb2+
4. compounds containing the sulfate ion(SO4^2-)
   exceptions: compound that contains Ag+,Hg2^2+,Pb2+,Ca2+,Sr2+ or Ba2+

Question 15

insoluble

Answer 15

1. compounds containing the carbonate ion(CO3^2-) phosphate ion(PO4^3-) chromate ion(CrO4^2-) or sulfide ion(S2-)
   exception: Li+, Na+,K+,Rb+,Cs+ or NH4+
2. compound containing the hydroxide ion (OH-)
   exception: Li+,Na+,K+,Rb+,Cs+,Ba+

Question 16

molecular equation

Answer 16

the chemical equation that treats all species as molecules

Question 17

total ionic equation

Answer 17

the chemical equation that explicitly shows the ions

Question 18

spectator ion

Answer 18

ions that do not participate in the ration they appertains on both sides of the total ionic equation

Question 19

acids

Answer 19

ability to dissolve metals. sour taste. turns litmus red

Question 20

bases

Answer 20

slippery feel, bitter taste, turns litmus blue

Question 21

acids

Answer 21

substances that contain H in the chemical formula and produces H+ ions when dissolved in water

Question 22

bases

Answer 22

substances that contains OH in the chemical formula and produces OH- ion when dissolved in water

Question 23

Limitations

Answer 23

1. restricts all acid-base reactions to water

2. excludes NHg and amines as bases

Question 24

acids

Answer 24

a proton donor

Question 25

bases

Answer 25

a proton acceptor

Question 26

Hydronium

Answer 26

H+ does not exist in the aqueous solution, in water, the H+ attaches to eater. H+ can be used for convenience, but it is H3O+

Question 27

Acid nomenclature

Answer 27

acidic compounds are named as acids if it is in solution. acids are named based on whether it contains oxygen or not. no oxygen hydro-anion-ic acid with oxygen anion acid -ite anion-ous acid -ate anion-ic acid

Question 28

polyphonic acid

Answer 28

acid with more than one ionizable proton

Question 29

monoprotic

Answer 29

acids with one ionizable proton

Question 30

diprotic

Answer 30

acids with two ionizable protons

Question 31

bronzed-lowry definition

Answer 31

proton accepts hydroxide compounds, metal oxides, ammonia ana amines

Question 32

strong acids

Answer 32

acids, that ionized completely

Question 33

strong bases

Answer 33

bases that ionize completely

Question 34

acid-base reactions

Answer 34

since acids are H+ donors and bases are H+ acceptors they are made to react together.

Question 35

Redox reactions

Answer 35

a chemical reaction in which electrons are transferred from one substance to another

Question 36

corrosion

Answer 36

the unwanted oxidation | 4Fe + 3O2--->2Fe2O3

Question 37

combustion reactions

Answer 37

2C8H8+25O2---->16CO2+18H20

Question 38

metabolic process

Answer 38

C6H12O6+6O2--->6CO2+6H2O+ATP

Question 39

voltaic cells

Answer 39

batteries | Zn+MnO2+H2O--->ZnO+Mn(OH)2

Question 40

matallurgy

Answer 40

extraction of metals from ore | Fe2O3+3CO--->2Fe+3CO2

Question 41

oxidation states

Answer 41

the hypothetical charge an atom would have if all bonds were ionic

Question 42

rules for oxidation states

Answer 42

1. the sum of the oxidation states must equal the net charge 2. for lone elements the os=charge 3. for ionic compounds, the charge of the ions are the os. 4. in compounds a. F is alway -1 b. H is usually +1 c.O is usually -2 except: hydride, peroxide's, superoxides

Question 43

os

Answer 43

the hypothetical charge an atom would have if all bonds were ionic

Question 44

reduce agent

Answer 44

a substance that causes another compound to be reduced, therefore itself is oxidized

Question 45

oxidizing agent

Answer 45

a substance that cause another compound to be oxidized, therefore itself is reduced

Question 46

Concentration of solutions

Answer 46

the amount of solute in solution can vary. one way of expressing this amount is through the unit of molarity Molarity, M: amount of solute, mol/ volume of solution L

Question 47

Dilutions

Answer 47

C1V1=C2V2. M1V1=M2V2 C1:mol/L V1: L=mol initially the amount of solute does not change when a solvent is added to dilute the solutions. but since the volume of solutions increases the concentration must decrease

Question 48

pH scale

Answer 48

in many applications the concentration of H+ ions is important often the concentration is small. pH=-log[H+]

Question 49

auto ionization of water

Answer 49

process is driven by hydrogen bonding

Question 50

Gravimetric analysis

Answer 50

analytical technique based on masses requires reactions to be completed

Question 51

tritration

Answer 51

an analytical technique for precisely determine the concentration or amount of solute in a sample by reacting it with a standard of known concentration

Question 52

equivalence point

Answer 52

the point in the titration in which the number of moles of titrant and moles of analyze are in stoichiometric equivalence

Question 53

end point

Answer 53

the point in the titration in which the indicator changes color indicating the stoppage of the titration