Chapter Five & Six
Ionic and Covalent Compounds
Chapters Five and Six
Ionic and Covalent Compounds
DEFINE THE FOLLOWING TERMS AND GIVE AN EXAMPLE
Element:
Ion:
Compound:
Polyatomic ion:
Page 1 of 80
Chapter Five & Six
Ionic and Covalent Compounds
SECTION 1: COVALENT BONDS (PG. 190 TO 191, 194-198)
Formed
by:
Covalent
Compounds
Determined
by:
Can be
either:
PROPERTIES
Page 2 of 80
Chapter Five & Six
Ionic and Covalent Compounds
CHARACTERISTICS OF IONIC COMPOUNDS pg. 171-175
Different from:
Formed by:
Ionic
Compounds
Characteristics/properties
Page 3 of 80
Chapter Five & Six
Ionic and Covalent Compounds
PRACTICE: ELECTRON CONFIGURATIONS FOR IONS
Element
Full Electron Configuration
H
1s1
He
1s2
Li
1s22s1
Al
1s22s22s1
P
1s22s22p63s23p3
Ar
1s22s22p63s23p6
Ca
1s22s22p63s23p64s2
Ga
1s22s22p63s23p64s23d104p1
Rb
1s22s22p63s23p64s23d104p65s1
I
1s22s22p63s23p64s23d104p65s24d105p5
Valence
Electron
Configuratio
n
Electrons it
will
gain/lose to
become
stable
Resulting
charge
Page 4 of 80
Chapter Five & Six
Ionic and Covalent Compounds
POLYATOMIC IONS
Hydroxide
Sulfate
Phosphate
Carbonate
Bicarbonate
OH-1
SO4-2
PO4-3
CO3-2
HCO3-1
Nitrate
Acetate
Cyanide
Ammonium
Iodate
NAME THE FOLLOWING COMPOUNDS:
Name of positive Name of negative
Compound
ion
ion
Change
ending?
NO3-1
C2H3O2-1
CN-1
NH4+1
IO3-1
Name of Compound
1. BaCO3
2. NaOH
3. Na2SO4
4. H2S
5. Ag2CO3
6. K3PO4
7. Na2CO3
8. MgCl2
9. CaO
10. (NH4)3PO4
11. Na2O
12. BeCl2
13. CaS
14. NaNO3
15. LiNO3
16. BaSO4
17. Mg(CH3COO)2
18. CaSO4
19. LiF
Page 5 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Write the formula in the correct box using the switcheroo method
Cl1-
(CO3)2-
(OH)1-
(SO4)-2
(PO4)3-
(NO3)1-
Na+
(NH4)1+
K+
Ca2+
Mg2+
Zn2+
Fe3+
Al3+
Co3+
Fe2+
H+
Page 6 of 80
Chapter Five & Six
Ionic and Covalent Compounds
PRACTICE PROBLEMS: LEWIS DOT DIAGRAMS FOR ELEMENTS
1. Complete this table:
Element
Valence
Electrons
Dot Diagram
O
Ar
S
Li
Si
C
P
Cl
H
Page 7 of 80
Chapter Five & Six
Ionic and Covalent Compounds
PRACTICE PROBLEMS: LEWIS DOT DIAGRAMS/ LEWIS DOT STRUCTURES
Draw Lewis Dot Structures for the following compounds
Molecule
Individual Dot
Diagrams
Total
Number of
Valence
Electrons
Determine
central
atom
Final structure
SCl2
AsF3
SiH4
CHF3
HS1-
Page 8 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Molecule
Individual Dot
Diagrams
Total
Number of
Valence
Electrons
Determine
central
atom
Final structure
NF41+
IO1-
PCl41+
CH4
Page 9 of 80
Chapter Five & Six
Ionic and Covalent Compounds
PRACTICE PROBLEMS: DOUBLE/TRIPLE BONDS
Draw Lewis Structures for the following molecules.
Molecule
Individual Dot
Diagrams
Total number
of Valence
Electrons
Determine
central
atom
Final structure
N2F2
O2
N2
CO2
NO1-
Page 10 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Practice Problems: Naming Covalent Compounds
Using the rules for covalent compounds, name the following compounds:
1. P2O5
2. N2O3
3. CF4
4. PI5
5. SO2
6. SO3
7. H2S
8. CCl4
9. CS2
10. P2O3
11. NO3
Using the rules for covalent compounds, write formulas for the following compounds:
1. boron trifluoride
2. Diphosphorus pentoxide
3. Antimony trichloride
4. Silicon dioxide
5. Carbon tetrachloride
6. Diphosphorus pentasulfide
Page 11 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Write the formulas for the following covalent compounds:
1)
antimony tribromide __________________________________
2)
hexaboron monosilicide __________________________________
3)
chlorine dioxide __________________________________
4)
hydrogen monoiodide __________________________________
5)
iodine pentafluoride __________________________________
6)
dinitrogen trioxide __________________________________
7)
Nitrogen trihydride __________________________________
8)
phosphorus triiodide __________________________________
Write the names for the following covalent compounds:
9)
P4S5 __________________________________
10)
O2 __________________________________
11)
SeF6 __________________________________
12)
Si2Br6 __________________________________
13)
SCl4 __________________________________
14)
CH4 __________________________________
15)
B2Si __________________________________
16)
NF3 _________________________________
Page 12 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Page 13 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Page 14 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Page 15 of 80
Chapter Five & Six
Ionic and Covalent Compounds
Page 16 of 80
Chapter Eight
Chemical Equations and Reactions
Chapter Eight:
Chemical Equations & Reactions
SECTION 1: DESCRIBING CHEMICAL REACTIONS (pg. 260 – 266)
1.
2.
3.
Different from:
Recognized by:
4.
Chemical Change
Represented by a:
Which include both:
Which often come with:
Page 17 of 80
Chapter Eight
Chemical Equations and Reactions
REVIEW: WRITING FORMULAS FOR COMPOUNDS
Write formulas for the following compounds (refer to Chapters 5 & 6 if you have problems):
IONIC COMPOUNDS
1. sodium chloride
5. ammonium phosphide
2. magnesium fluoride
6. ammonium phosphate
3. rubidium oxide
7. magnesium nitrate
4. calcium carbonate
COVALENT COMPOUND
8. trisulfur dioxide
11. boron triiodide
9. carbon monoxide
12. dinitrogen pentabromide
10. carbon tetrachloride
MIXED IONIC AND COVALENT
1. carbon dioxide
10. potassium oxide
2. iron (III) chloride
11. sodium fluoride
3. phosphorus trichloride
12. sodium carbonate
4. sodium oxide
13. sulfur trioxide
5. magnesium hydroxide
14. lithium bromide
6. diphosphorus pentoxide
15. magnesium oxide
7. calcium chloride
16. ammonium chloride
8. water
9. barium sulfate
Page 18 of 80
Chapter Eight
PRACTICE PROBLEMS: WRITING WORD EQUATIONS
For each of the following problems complete the following tasks.
A. Write the word equation
B. Convert the word equation into chemical formulas
C. Identify the type of reaction
D. Balance the reaction
1. When dissolved beryllium chloride reacts with dissolved silver nitrate in water, beryllium nitrate and
silver chloride powder are made.
A.
B.
C.
D.
2. When isopropanol (C3H8O) burns in oxygen, carbon dioxide and water are produced.
A.
B.
C.
D.
3. When dissolved sodium hydroxide reacts with sulfuric acid (H2SO4), sodium sulfate and water are
formed.
A.
B.
C.
D.
Page 19 of 80
Chapter Eight
4. When fluorine gas is put into contact with calcium metal at high temperatures, calcium fluoride
powder is created in an exothermic reaction.
A.
B.
C.
D.
5. When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed.
A.
B.
C.
D.
6. Hydrogen and nitrogen react together to produce ammonia gas (NH3).
A.
B.
C.
D.
Page 20 of 80
Chapter Eight
7. Propane (C3H8) burns in oxygen to produce carbon dioxide and steam (water vapor).
A.
B.
C.
D.
8. When heated, aluminium reacts with solid copper (I) oxide to produce copper metal and aluminium
oxide.
A.
B.
C.
D.
9. Potassium oxide is not a stable compound. In the presence of water, it readily converts into
potassium hydroxide.
A.
B.
C.
D.
Page 21 of 80
Chapter Eight
10. Sodium chloride and silver nitrate combine to form silver chloride and sodium nitrate.
A.
B.
C.
D.
11. Sodium bicarbonate decomposes, resulting in the formation of solid sodium carbonate as well as
water vapor and carbon dioxide gas.
A.
B.
C.
D.
12. Poisonous hydrogen sulfide gas can be neutralized with sodium hydroxide. This reaction produces
water and sodium sulfide.
A.
B.
C.
D.
Page 22 of 80
Chapter Eight
13. Disposable lighters use butane, C4H10, as a fuel. The complete combustion of butane requires a
supply of oxygen and results in the formation of carbon dioxide and water vapor.
A.
B.
C.
D.
14. Barium chloride combines with sodium carbonate to form barium carbonate and sodium chloride.
A.
B.
C.
D.
15. Sodium metal reacts violently with water. The reaction results in the formation of sodium hydroxide
and flammable hydrogen gas, which often bursts into flame during the reaction.
A.
B.
C.
D.
Page 23 of 80
Chapter Eight
16. Chlorine gas reacts with sodium oxide to produce oxygen gas and sodium chloride
A.
B.
C.
D.
17. Solid zinc metal combines with chlorine gas to form zinc chloride
A.
B.
C.
D.
18. Sodium bicarbonate (NaHCO3) decomposes to form solid sodium carbonate, carbon dioxide gas
and water.
A.
B.
C.
D.
Page 24 of 80
Chapter Eight
SECTION TWO: BALANCING CHEMICAL EQUATIONS (PG. 267 TO 274)
Which means:
Matter is conserved
Therefore:
By changing:
Never by:
These indicate:
These indicate
Page 25 of 80
Chapter Eight
MORE TYPES OF CHEMICAL REACTIONS TO IDENTIFY AND BALANCE
1. _____ Fe + _____O2 _____ Fe2O3
2. _____Zn + _____HCl  _____ZnCl2 + _____H2
3. _____NiCl2  _____Ni + _____Cl2
4. _____C + _____H2 + _____O2  _____C2H6O
5. _____C12H22O11  _____C + _____H2O
6. _____LiI + _____Pb(NO3)2  _____LiNO3 + _____PbI2
7. _____CdCO3  _____CdO + _____CO2
8. _____Cl2 + _____KBr  _____KCl + _____Br
9. _____BaCl2 + _____KIO3  _____Ba(IO3)2 + _____KCl
10. _____PH3 +_____ O2  _____P2O5 + _____H2O
11. _____C3H5ON + _____O2  _____CO2 + _____H2O + _____NO2
12. _____Hg(NO3)2  _____HgO + _____NO2 + _____O2
13. _____CH3NO2 + _____O2  _____NO2 ____CO2 + _____H2O
14. _____Al + _____S8  _____Al2S3
15. _____B2S3 + _____H2O  _____H3BO3 + _____H2S
16. _____NH3 + _____Na  _____H2 + _____NaNH2
17. _____Li3N + _____H2O  _____NH3 + _____LiOH
18. _____CCl4 + _______O2  _____CCl2O +_____ Cl2
19. _____K + _____NH3  _____KNH2 + _____H2
Page 26 of 80
Chapter Eight
Chemical Reactions:
____________________________________________________________________
Evidence of a Chemical Reaction
1. ______________________________
4. ______________________________
2. ______________________________
5. ______________________________
3. ______________________________
Chemical Reactions: ___________________________________
Two Parts to a Chemical Equation
1. ______________________
2. ______________________
_____________________  ______________________
Writing formulas
Ionic Compounds
Covalent Compounds
__________and ______________
____________and ___________
1. ______________________
1. ________________________
2. ______________________
2. ________________________
3. ______________________
3. ________________________
Examples:
Examples:
Sodium Chloride
Diphosphorus pentoxide
Gallium nitride
Boron trichloride
Diatomic Molecules: _______________________________________________________________
1)
2)
3)
4)
5)
6)
7)
___________________
___________________
___________________
___________________
___________________
___________________
___________________
Page 27 of 80
Chapter Eight
Word Equations to Symbol Equations
Example: Isopropanol (C3H8O) burns in oxygen, carbon dioxide and water are produced.
Five Types of Reactions
1) Combination: ________________________________
Example:
2) Decomposition: ________________________________
Example:
3) Single Replacement:________________________________
Example:
4) Double Replacement:________________________________
Example:
5) Combustion: ________________________________
Example:
Chemical Equations
Provides information about the reactions
 ___________________________________________________________
 ____________________________________________________________
 ____________________________________________________________
Law of Conservation of Matter
Matter cannot be _______________ or ________________.
____________________ = _________________________
Balancing Equations
 Never mess with _____________________
 ALWAYS use _________________________
Page 28 of 80
Chapter Eight
Examples:
Magnesium
+
Hydrogen Chloride 
hydrogen +
magnesium chloride
____NCl3  ______ N2 + _____Cl2
___ Al2(SO4)3 + ___ Ca(OH)2  ___ Al(OH)3 + ___ CaSO4
Activity Series:
________________________________________________________________________
 Elements arranged _____________________________________
 Most ____________ on TOP

Everything below an element _________________________
Page 29 of 80
Chapter Eight
The Mole and Chemical Composition
CONVERSION FACTORS
USE CONVERSION FACTORS TO SOLVE THE FOLLOWING:
1. How many feet are in 2.6 miles? (1 mile = 5280 feet) (13728)
2. How many ounces are in 6.3 gallons (128 ounces in 1 gallon) (806.4)
3. How many troy ounces in 15 pounds (1 troy ounce = 0.07 pounds) (214)
4. How many seconds in 17 hours? (61,200)
FACTOR LABEL
PURPOSE: PROBLEM SOLVING USING THE FACTOR-LABEL METHOD.
Simple Conversions:
1. How much does a person weigh in kilograms if that person weighs 128 lbs? (58)
2. How many centimeters are there in 16.2 inches? (41)
3. Express the volume of a 250 ml flask in liters. (0.250)
4. Express the volume of a 250 ml in quarts. (0.265)
5. How many grams are contained in 7.0 lbs. (3175)
6. Convert 3.4 miles to kilometers. (5.5)
7. Convert 3.4 miles to meters. (5470.6)
8. If an automobile is traveling 55 mi/hr, how fast is it traveling in kilometers per hour? (88)
Page 30 of 80
Chapter Eight
9. A crucible weighs 57 grams. Express its mass in ounces. (2)
Multiple Conversions:
10. Calculate the number of minutes in 5 days. (7,200)
11. Calculate the number of kilometers in 13,500 yards. (104)
12. How many seconds are there in seven hours? (25,200)
13. A bullet fired from a gun travels at a speed of 1500 ft each second. What is this speed in
miles per hour? (1023)
14. Calculate the number of milliliters contained in a 2 pint carton of milk. (946)
15. How many hours are there in three years? (26,280)
16. A baseball leaves a bat at a speed of 45 m/sec. How fast is the ball traveling in miles per
hour?(101)
17. How many pints of water are contained in 57,200 cm3. (1 cm3 = 1 ml) (121)
Conversions involved in word problems
18. What is the cost of a pair of socks if a package of socks costs $4.89 and there are three
pairs of socks per package? (1.63)
19. What is the cost to drive from San Francisco to Los Angeles, a distance of 405 miles, if the
cost of gasoline is $1.24 per gallon and the automobile gets 18 miles per gallon of fuel?
(27.90)
20. Determine the price per pound of paper, if each sheet of paper weighs 0.50 ounces, there
are 500 sheets of paper in a ream, and a ream of paper can be purchased for $6.25. (0.40)
Page 31 of 80
Chapter Eight
21. How many oranges are in a crate if the price of a crate of oranges is $8.85 and the price of
oranges is $0.59 per pound. On average, there are three oranges per pound. (45)
22. How many cars are there in a freight train if it takes the entire train 3 minutes to pass a
station as it travels 45 miles per hour. Each car is 50 ft. long. (238)
23. How many dozen eggs would need to be ordered for one week if a restaurant serves 45
people every morning, and on average, two thirds of the people order two eggs and one
third of the people order the three-egg omelet? (Hint: make this a two part problem) (62)
24. Using the information in question 23, how much will the eggs cost, in dollars, if eggs are
selling of 69 cents per dozen? (42.78)
25. If a car travels 40.75 feet in one second, how many miles will it travel in exactly one hour?
26. A flock of birds consumes 40.0 pounds of seed in four days. How many weeks will it take
for the birds to consume 1400 kg of seed?
27. The approximate total number of minutes for a semester of school (including evenings and
weekends) is 181,440. How many weeks is this?
28. Sound travels approximately at a rate of 344 meters per second through air. Determine
this rate in miles per hour.
29. A high school senior was applying to college and wondered how many applications she
needed to send. Her counselor explained that with the excellent grade she received in
chemistry she would probably be accepted to one school out of every three to which she
applied. [3 applications = 1 acceptance] She immediately realized that for each application
she would have to write 3 essays, [1 application = 3 essays] and each essay would require
2 hours work [1 essay = 2 hours]. Of course writing essays is no simple matter. For each
hour of serious essay writing, she would need to expend 500 calories [1 hour = 500
calories] which she could derive from her mother's apple pies [1 pie = 1000 calories]. Her
mother will bake here one apple pie for every time she cleans here room. How many
times would she have to clean her room in order to gain acceptance to 10 colleges?
Page 32 of 80
Chapter Eight
30. A case of apples costs $16.00. What is the cost for twenty apples if a case contains 192
apples?
31. Consider the following: 3 bushels = 1 sack, 4 pecks = 1 bushel, 2 gallons = 1 peck. If the
cost of a gallon of apples equals $4.50. How much would 20 sacks of apples cost?
32. Two dozen dimes will create a stack of approximately 1 inch in height. Nickels are as thick
as 1-¾ dimes. How many nickels would you have if your stack reached 6 feet?
33. The recent rainfall averages 2.7 inches per day. In my back yard sits a wading pool 3 feet
in depth. If I were cheap enough to let Mother Nature fill my pool for me, how many weeks
would I have to wait, assuming it rains 3 days a week.
34. Walking burns 550 Calories an hour. A bacon, egg and cheese croissant contains 364
Calories. How many hours (each month) must I walk to work off a month’s worth of
croissants? I each croissants 3 times a week. Assume that one month = 4 weeks
35. How many minutes will it take to drive to Los Angeles from San Francisco if an
average speed of 72 mi/hr is maintained? The distance between the two cities is
350 kilometers.
Page 33 of 80
Chapter Eight
ATOM COUNT
Compound
H3PO4
# of atoms/molecule
# molecules/mole
8
6.02  1023
Zn3(PO4)2
CuSO4
Fe2(CO3)3
NaNO3
HOCl
H2Se
CS2
Na2PO4
Mn2O3
KMnO4
Ti2O3
Sc2O3
Page 34 of 80
# atoms/mole
H : 3(6.02  1023) =
P : 6.02  1023
O : 4(6.02  1023) =
Chapter Eight
Molar Mass
Calculate the molar mass for each of the following compounds.
1. N2H4 (32)
2. H3PO4
3. Zn3(PO4)2 (386)
4. CuSO4
5. Fe2(CO3)3 (292)
6. NaNO3
7. HOCl (52)
8. H2Se
9. CS2 (76)
10. Na2PO4
11. Mn2O3 (158)
12. KMnO4
13. Ti2O3 (144)
14. Sc2O3
15. C6H12O6 (180)
16. Mo(CO)6
17. NaC2H3O2 (82)
18. AgIO3
19. RaSO4 (322)
20. PbSO4
21. SrCrO4 (204)
22. Sr(NO3)2
23. Al2(SO4)3 (342)
24. (NH4)2SO4
Page 35 of 80
Chapter Eight
PRACTICE PROBLEMS: MOLAR CONVERSIONS FOR ELEMENTS
Calculate the mass in grams of each of the following:
1. 5.0 moles of C (60 )
2. 8.00 moles of Al
3. 10.5 moles of O2 (336)
4. 200 moles of Cl2
5. 4.00 moles of Hg (802)
6. 7.00 moles of I2
7. 6.20 moles of Mg (149)
8. 9.20 moles of Fe
Calculate the number of moles in the following:
1. 800 g of Ca (20)
2. 280 g of Fe
3. 560 g of Br (7.0)
4. 72 g Mg
5. 66 g of Mn (1.2)
6. 93 g of P
7. 80 kg of S (2500)
8. 1035 g of Pb
Page 36 of 80
Chapter Eight
Calculate the mass in grams of each of the following:
1. 5.00 moles of ZnO (405)
2. 12.0 moles of HCl
3. 6.00 moles of H2SO4 (588)
4. 7.500 moles of sugar, C12H22O11
5. 200 moles of Al2O3 (20,400)
6. 40.0 moles of Na2CO3
7. 80.0 moles of methane (1280)
8. 8.2 moles of CaCO3
Calculate the number of moles in each of the following:
1. 400 grams of NaOH (10)
2. 2700 grams of H2O
3. 814 grams of Ca(OH)2 (11.0)
4. 3.0 kilograms of CaCO3
Calculate the following:
1. mass of 192 moles of HCl (6912)
3. mass of 17.2 moles of Na2O (1067)
2. moles in 510 grams of Al2O3
4. moles in 36 kilograms of CaS
Page 37 of 80
Chapter Eight
More Mole Map Problems
1) Calculate the number of particles in
2.50 moles of Neon, Ne (1.51  1024)
0.050 moles of iron, Fe (3.0  1022)
2) Calculate the number of moles in
9.03 X 1023 atoms of Cu
3.76 X 1025 molecules of SO2
8.6 X 1018 electrons
3) Calculate the number of molecules in
12.5 g of nitrogen, N2 (2.69  1023)
0.76 g of ammonia, NH3 (2.7  1022)
0.60 g of hydrogen, H2 (1.8  1023)
4) Calculate the mass of
4.25 X 1024 atoms of C
6.02 X 1021 molecules of H2O
one billion atoms of Zn
one atom of U
Page 38 of 80
Chapter Eight
5) Calculate the mass of
2.00 moles of water, H2O (36.0)
4.38 moles of chlorine, Cl2 (311)
0.025 moles of ammonia, NH3 (0.43)
1.8 moles of oxygen, O2 (58)
6) How many moles are in 15 grams of lithium?
7) How many grams are in 2.4 moles of sulfur? (77)
8) How many moles are in 9.8 grams of calcium?
9) How many grams are in 4.5 moles of sodium fluoride, NaF? (190)
10) How many moles are in 68 grams of copper (II) hydroxide, Cu(OH)2?
11) How many grams are in 2.3 x 10-4 moles of calcium phosphate, Ca3(PO3)2? (0.064)
12) What mass of carbon contains the same number of atoms as 1.008g of hydrogen?
13) What mass of oxygen contains the same number of atoms as 14.01g of nitrogen? (16.00)
14) What mass of nitrogen contains the same number of atoms as 48g of oxygen?
15) Which weighs more, 1 mole of helium atoms or 0.5 mole of carbon atoms?
Page 39 of 80
Chapter Eight
Page 40 of 80
Chapter Eight
Page 41 of 80
Chapter Eight
Page 42 of 80
Chapter Eight
Page 43 of 80
Chapter Nine
Stoichiometry
Chapter Nine
Stoichiometry
SECTION 1: CALCULATING QUANTITIES (pg. 302-303)
Balanced
Equation
Provides you with
Which give you the
amount of:
Small scale
Normal/everyday scale
OR
Which can give you the:
(most important part)
Which tells you:
Page 44 of 80
Chapter Nine
Stoichiometry
PRACTICE PROBLEMS: MOLE RATIOS (CONVERSIONS) FROM BALANCED EQUATIONS.
For each word equation below, write a balanced equation then write a conversion factor for the
change requested.
1. Potassium + Sodium Sulfide  Potassium Sulfide + Sodium
2K + Na2S  K2S + 2Na
a. Write a mole ratio for potassium to potassium sulfide
b. Write a mole ratio for sodium sulfide to potassium.
2. Ammonium Nitrate + Magnesium Oxide  Magnesium Nitrate + Ammonium Oxide
2 NH4NO3 + MgO  Mg(NO3)2 + (NH4)2O
a. Write a mole ratio for magnesium nitrate to magnesium oxide.
b. Write a mole ratio for ammonium nitrate to magnesium nitrate
3. Hydrogen + Oxygen  Water
____H2 +
_____ O2
 ____ H2O
a. What is the mole ratio used to change from oxygen to water?
b. What is the mole ratio used to change from hydrogen to oxygen?
4. Lithium Carbonate + Sodium Chloride  Sodium Carbonate + Lithium Chloride
___Li2CO3 + ____NaCl  ____ Na2CO3 + ____ LiCl
a. Mole ratio for sodium chloride to sodium carbonate.
b. Mole ratio of lithium carbonate to sodium carbonate.
5. Aluminum Oxide  Aluminum and Oxygen
2 Al2O3  4 Al + 3 O2
a. Mole ratio from aluminum oxide to aluminum.
b. Mole ratio from moles of oxygen to moles of aluminum oxide.
Page 45 of 80
Chapter Nine
Stoichiometry
Stoichiometry Questions
For each problem listed, write a balanced equation and then answer the questions that follow.
1. Lead (IV) Sulfate + Lithium Chloride  Lithium Sulfate + Lead (IV) Chloride
_____Pb2(SO4)4 + __8__ LiCl  __4__ Li2SO4 + _2__PbCl4
a. What is the mole ratio for lead sulfate to lithium chloride?
b. If I have two moles of lead sulfate, how many moles of lithium chloride will I need
to react?
2. Use the equation from question #1 to answer these questions:
a. How many moles of lead sulfate are needed to react with 2 moles of lithium
chloride?
b. How many moles of lead chloride will be produced if I have 1 mole of lead sulfate
to react?
c. Use factor label or a proportion to determine how many moles of lithium sulfate will
form if I have 0.67 moles of lithium chloride.
d. How many moles of lead chloride will be produced if I have 0.55 moles of lead
sulfate to start with?
3. Aluminum + hydrogen sulfate  Aluminum sulfate + hydrogen gas
____Al + ____ H2SO4  ____ Al2(SO4)3 + ____ H2
a. How many moles of aluminum will react with 3 moles of hydrogen sulfate?
b. How many moles of aluminum sulfate will form when I react 0.87 moles of
hydrogen sulfate?
c. How many moles of hydrogen do I have, if I have 1.22 moles of aluminum?
d. How many moles of aluminum will I need to react with 0.27 moles of hydrogen
sulfate?
Page 46 of 80
Chapter Nine
Stoichiometry
PRACTICE PROBLEMS: MORE MOLE-MOLE STOICHIOMETRY
Balance the following equations and then convert as requested.
1. Iron (III) Nitrate + Copper (I) Hydroxide  Iron (III) Hydroxide + Copper (I) Nitrate
_____ Fe(NO3)3 + ____ CuOH  ____ Fe(OH)3 + ____ CuNO3
a. How many moles of iron hydroxide can be produced from 2.6 moles of copper
hydroxide? (0.87)
b. How many moles of iron nitrate are needed to react with 0.5 moles of copper
hydroxide? (0.17)
2. Barium Oxide + Silver Nitrate  Silver Oxide + Barium Nitrate
____ BaO + _____AgNO3  ____Ag2O + ____ Ba(NO3)2
a. How many moles of silver oxide are produced if 3.5 moles of silver nitrate are
used? (1.75)
b. How many moles of barium nitrate are produced if 1.7 moles of silver oxide are
also produced? (1.7)
3. Ammonium Phosphate + Barium Chloride  Ammonium Chloride + Barium Phosphate
____ (NH4)3PO4 + ____ BaCl2  ____ NH4Cl + ____ Ba3(PO4)2
a. How many moles of barium chloride will react with 5 moles of ammonium
phosphate? (7.5)
b. How many moles of ammonium chloride are produced from 7.5 moles of
ammonium phosphate? (22.5)
4. Lithium + Strontium Sulfide  Lithium Sulfide + Strontium
____ Li + ___ SrS  _____ Li2S + ____ Sr
a. How many moles of strontium are produced when 2.5 moles of lithium are
reacted? (1.25)
b. How many moles of lithium sulfide are reacted when 0.57 moles of strontium
sulfide are used up?
Page 47 of 80
Chapter Nine
Stoichiometry
5. Methane (CH4) + Oxygen  Carbon Dioxide and Water
CH4 + 2O2  CO2 + 2 H2O
a. How many moles of water are produced from burning 2 moles of methane? (4 mol)
b. How many moles of oxygen are consumed to produce 10 moles of water? (20 mol)
6. Ammonia (NH3) Nitrogen + Hydrogen
____ NH3  ____ N2 + ____ H2
a. What quantity (in moles) of hydrogen is released when 4.1 moles of ammonia
decomposes? (6.15)
b. How many moles of nitrogen are produced when 3 moles of hydrogen is also
produced? (1 mol)
Page 48 of 80
Chapter Nine
Stoichiometry
GETTING TO MOLES (PG. 304-310)
Moles is a central unit, crucial to stoichiometry. But not every problem will give
you moles. In this map, show the conversions that will allow you to “get to”
moles so that you can perform stoichiometry.
Which you get
from:
Which you get
from:
Convert, using:
Convert, using:
If you are given:
If you are given:
Moles
If you are given:
Which you get
from:
Convert,
using:
Page
49 of 80
Which you get
from:
Chapter Twelve
Gases
Even More Complex Stoichiometry Problems
Use this balanced equation for questions 1 to 3:
2NaI + BaS  BaI2 + Na2S
1. If I have 0.893 moles of BaS, how many grams of barium iodide can I produce?
2. Calculate how many moles of barium sulfide I need, if I have 177 grams of sodium iodide.
3. If 19 grams of barium iodide is produced, how many moles of sodium sulfide are also
produced.
Balance this equation, and use it for questions 4 to 7:
_____Ga + _____S  _____Ga2S3
4. Calculate the grams of gallium sulfide produced from 19 grams of sulfur.
5. Determine the grams of sulfur needed to produce 125 grams of gallium sulfide.
6. How many grams of sulfur are needed to react with 1.33 moles of gallium?
7. What amount (in grams) of gallium sulfide is produced if 1.77 moles of gallium is used?
Balance the equation. This will be used to answer questions 8 through 10.
_____C5H12 + _____O2  _____ CO2 + _____ H2O
8. Calculate the moles of carbon dioxide formed from 32 moles of oxygen.
9. Determine the grams of water formed when 124 grams of C5H12 are burned.
10. How many grams of oxygen are needed to burn 36 grams of C5H12.
Page 50 of 80
Chapter Twelve
Gases
Page 51 of 80
Chapter Twelve
Gases
Page 52 of 80
Chapter Twelve
Gases
Chapter Twelve
Gases
SECTION ONE: CHARACTERISTICS OF GASES (pg. 416-422)
Properties
of Gases
GASES
Gas and
Pressure
Kinetic
Molecular
Theory
Gas
Relationships
Page 53 of 80
Chapter Twelve
Gases
PRACTICE PROBLEMS: PRESSURE * TEMPERATURE CONVERSIONS
Perform the following conversions:
Remember: 101.325 kPa = 760 mmHg = 1 atm
C +273 = Kelvin
1. 520 mmHg =
atm
2. 75 kPa =
mmHg
3. 93.7 kPa =
atm
4. 97.25 kPa =
Pa
5. 120,354 Pa =
atm
6. 323 mmHg =
kPa
7. 25 C =
K
8. –30 C =
K
9. 19 C =
K
10. 323 K =
C
11. 0 K =
C
12. 255 K =
C
Page 54 of 80
Chapter Twelve
Gases
GAS -CONCEPTS - PRACTICE PROBLEMS
1. There are three cylinders drawn in the space below. The sizes of the cylinders can be
changed by raising or lowering the piston. The volumes of the cylinders are labeled. Draw
15 particles in each cylinder to represent the particles of a gas. Remember that a gas
expands to fill its container.
2. How do the numbers of particles in each cylinder vary with the volume of the cylinder?
3. How does the volume of the cylinder affect the pressure within the cylinder? Explain your
answer.
Page 55 of 80
Chapter Twelve
Gases
4. Three balloons have been drawn in the space above. Initially all of the balloons were
exactly the same size and they were filled with exactly the same amount of air. One
balloon has been heated, one balloon is at room temperature and one balloon has been
cooled. Fill each balloon with 15 particles to represent the particles of a gas. Then label
which balloon has been heated, which is at room temperature and which has been cooled.
5. In which balloon are the particles the farthest apart? Why?
6. Make a general statement that reflects how the temperature of a gas is related to its
volume.
7. As the temperature of a gas decreases, its volume decreases until a temperature of
absolute zero (O K) is reached. Using the kinetic molecular theory, explain why the volume
of a gas should eventually reach 0L as the temperature decreases. Be sure to also
mention the speed of particles at temperatures above and equal to absolute zero.
Page 56 of 80
Chapter Twelve
Gases
READING: GAS LAWS (PG. 423-432)
Using the equation:
Using the equation:
Which relates the two properties:
Which relates the two properties:
Gas Laws
Which relates the two properties:
Using the equation:
Which relates the two properties:
Using the equation:
Page 57 of 80
Chapter Twelve
Gases
Direct relationship
Inverse relationship
Amount constant
Temperature
constant
Pressure constant
Involves change in
amount
Involves volume
change
Involves pressure
change
Involves temperature
change
COMBINED GAS LAW PRACTICE
Boyles
Charles
Avogadro’s
Gay-Lussac
P1
V1
T1
P2
1
1.5 atm
3.0 L
20 C
2.5 atm
2
720 torr
256 ml
25C
3
600 mmHg
2.5 L
22C
760 mmHg
1.8L
750 ml
0.0C
2.0 atm
500 ml
25C
101 kPa
6.0 L
471 K
900 torr
225 ml
150C
2.5 L
30C
100 ml
75C
4
5
95 kPa
4.0 L
6
650 torr
7
850 mmHg
1.5 L
8
125 kPa
125 ml
100C
V2
30C
250 ml
15C
100 kPa
T2
50C
Page 58 of 80
Chapter Twelve
Gases
PRACTICE PROBLEMS: GAS LAW PROBLEMS
1. A sample of carbon dioxide occupies a volume of 3.50 liters at 1.5 atm pressure. What
pressure would the gas exert if the volume were decreased to 2.00 L? (2.625 atm)
2. A 2.0 liter container of nitrogen had a pressure of 3.2 atm. What volume would be
necessary to decrease the pressure to 1.0 atm? (6.4)
3. Ammonia gas occupies a volume of 450 ml at a pressure of 0.89 atm. What volume will it
occupy at a standard pressure? (400.5)
4. A 175 ml sample of neon had its pressure changed from 0.6 atm to 1.4 atm. What is its
new volume? (75)
5. A sample of hydrogen at 1.5 atm had its pressure decreased to 0.50 atm producing a new
volume of 750 ml. What was its original volume? (250)
6. Bacteria produce methane gas in sewage treatment plants. This gas is often captured or
burned. If a bacterial culture produces 60.0 mL of methane gas at 1.45 atm, what volume
would be produced at 1 atm? (87)
7. At one sewage treatment plant, bacteria cultures produce 1000 L of methane gas per day
at 10 atm pressure. What volume tank would be needed to store one day’s production at
5.0 atm. (2,000)
8. Hospitals buy 400 L cylinders of oxygen gas compressed at 150 atm. They administer
oxygen to patients at 3.0 atm in a hyperbaric oxygen chamber. What volume of oxygen
can a cylinder supply at this pressure?
Page 59 of 80
Chapter Twelve
Gases
9. A 1.00 L balloon is filled with helium at 1.20 atm. If the balloon is squeezed into a 0.500 L
what is the new pressure?
10. A gas measured a volume of 100 mL under pressure of 0.75 atm. What would the volume
be under a pressure of 1.2 atm with constant temperature?
11. A sample of gas is confined to a 100 ml flask under a pressure of 0.80 atm. If this same
gas were transferred to a 50 ml flask, what would be the resulting pressure?
12. When measured at a temperature of 60°C, a volume of gas is 600 mL. What is the volume
at 10°C? (510)
13. If 105 ml of oxygen at 25°C were heated until its volume expanded to 120 ml, what would
be its final temperature? (341)
14. What will be the volume of 4°C of a quantity of gas that occupies 1L at 20°C? (0.95)
15. A quantity of hydrogen has a volume of 103 ml at a temperature of 20°C. To what
temperature would this gas need to be cooled to reduce the volume to 92 ml? (262)
16. The temperature of a gas changes to 14.8°C from its original value of 1.6°C. If the original
volume was 16.2 ml, what is the final volume of the gas at the new temperature? (16.98)
17. If 136 ml of nitrogen at 25°C is cooled to 0°C, what will be the new volume? (124.6)
Page 60 of 80
Chapter Twelve
Gases
1. It is much easier to slice a piece of pie with the edge of a sharp knife than
with the edge of a pencil. Explain this observation in terms of applied
pressure.
2. Heavy vehicles that must move easily over loose sand are often equipped
with special tires.
a. Would you expect these tires to be wide or narrow?
b. Explain your answer using the concept of pressure.
Imagine that you cause 8 to 10 highly elastic, small “super-bounce” balls to bounce
around inside a box that you steadily shake; this serves as an analogy for gas
molecules randomly bouncing around inside a sealed container. The balls bounce
randomly around inside the box.
1. Decide which of these four gas variables- volume, temperature, pressure, or
number of molecules- best matches each of the following factors, and explain
each choice:
a. The number of super-bounce balls inside the box
b. The size of the box
c. The vigor with which you shake the box
d. The number and force of collisions of the randomly moving superbounce balls with the box walls
2. How does each of the following changes relate to what you learned about
gases and the kinetic molecular theory?
a. The vigor shaking and the number of super-bounce balls remain the
same, but the size of the box is decreased.
b. The size of the box and the number of super-bounce balls remain the
same but the shaking becomes more vigorous.
c. The size of the container and the vigor of shaking are kept the same,
but the number of super-bounce balls is increased.
Page 61 of 80
Chapter Twelve
Gases
Page 62 of 80
Chapter Twelve
Gases
Page 63 of 80
Types
of
Matter
Semantic
Map
Can be separated by density
Can be separated through boiling
Created through physical means
Created through a chemical reaction
Differences can be seen with the
naked eye
Can be separated through filtration
Can be separated through physical
means
Can be separated through chemical
means
Mixture
Pure
Contains 2 or more elements in a
definite ratio
Contains 2 or more substances in
which the amount can vary
Contains only one type of element
Chapter Thirteen
Solutions
Chapter Thirteen
Solutions
REVIEW: TYPES OF MATTER
ELEMENT
Compound
Heterogeneous
Mixture
Homogeneous
Mixture
Solution
Suspension
Colloid
Page 64 of 80
Chapter Thirteen
Solutions
SECTION ONE: WHAT IS A SOLUTION? (pg. 454 – 459)
Described as:
Described as:
Type
Type
Described as:
Type
Mixtures
Can be separated by:
Which is used when:
Page 65 of 80
Chapter Fifteen
Acids and Bases
PRACTICE: CONCENTRATION PROBLEMS I
Note: 1 g of water = 1 mL of water
1. Calculate the percent solution for a solution that is 25 grams solute and 125 grams solvent.
2. Determine the concentration of a solution (in ppm) if the solute is 170 grams and the
solvent is 50 grams.
3. What is the molarity of a solution which contains 55 grams of NaCl and 750 ml of solution?
4. Calculate the concentration (in ppt) of a solution which contains 25 grams of magnesium
chloride (MgCl2) dissolved in 912 ml of water.
5. Calculate the molarity of a solution of MgI2 if 45 grams is dissolved in 200 ml of solution.
6. What is the percent solution of a compound if 23 grams is dissolved in 150 ml of water?
7. 192 grams of Mg(NO3)2 is dissolved in 1200 ml of water.
a. Calculate this concentration in pph.
b. Calculate the molarity of this solution.
8. If 8.0 grams of NaOH is dissolved in 125 ml of water, what is the molarity of the resulting
solution?
9. If 53 grams of PbCl2 is dissolved in 256 ml of water
a. Calculate the concentration using percent solution.
b. Determine the molarity of this solution.
Page 66 of 80
Chapter Fifteen
Acids and Bases
10. Calculate the molarity of a solution with 93 grams of AgC2H3O2 dissolved in 150 grams of
water.
11. Determine the grams of solution dissolved if 200 milliters of a calcium oxide solution has a
molarity of 3.0 M.
12. What amount of sodium chloride has been dissolved if a 250 ml solution of sodium chloride
has a concentration of 57 pph?
13. How many grams of Kr will be needed to prepare 1500 ml of a 1.5 M solution?
14. A 1.5 M solution contains 0.27 moles of FeCl3. What is the volume of the solution in liters?
15. A 2.5 M solution of FeCl3 contains 33 grams of iron chloride. What is the volume of the
solution in liters?
16. How many grams of HCl are in 65 ml of a 1.50 M solution?
17. What volume of 0.200 M CaCl2 solution can be prepared from 1.11 grams of solid CaCl2?
18. What is the molarity of a NaCl solution that was prepared by adding 23.4 grams of NaCl to
100 ml of water?
Page 67 of 80
Chapter Fifteen
Acids and Bases
SATURATED/UNSATURATED/SUPERSATURATED PROBLEMS
Complete the following problems:
Note: 1 g water = 1 ml water
1. Sodium chloride has a solubility of 35.9 g/100 ml water. Use this information to determine
if each of the following solutions is saturated, unsaturated or supersaturated.
a. A solution of sodium chloride contains 85 grams dissolved in 150 ml of water.
b. Twenty five grams of sodium chloride is dissolved in 75 grams of water.
c. A salt water solution contains 135 grams of NaCl dissolved in 750 grams of water.
2. Silver Nitrate has a solubility of 152 g/100 ml of water. Use this information to determine if
each of the following solutions is saturated, unsaturated or supersaturated.
a. A solution of silver nitrate is created by dissolving 75 grams in 95 ml of water.
b. 195 grams of silver nitrate is mixed in 200 grams of water.
c. A silver nitrate solution is formed by mixing 500 grams of silver nitrate with 750 ml
of water.
3. Copper chloride is not very soluble in water. It has a solubility of 0.0062 g/100 ml of
water. Use this information to determine if each of the following solutions is saturated,
unsaturated or supersaturated.
a. 0.076 g of copper chloride is dissolved in 150 grams of water.
b. 35 grams of copper chloride in 1.2 L of water.
c. 0.0124 in 175 ml of water.
Page 68 of 80
Chapter Fifteen
Acids and Bases
Remember to refer to the solubility graph study guide for hints on using a solubility
graph.
1. Why do the temperatures on the graph only go from 0º C to
100º?________________________________________________________________
2. Which substance is most soluble at 60º C ?________________________________
3. Which two substances have the same solubility at 80º C
?_____________________________________________________
4.Which substance’s solubility changes the most from 0º C to 100º C
?_________________________
5.Which substance’s solubility changes the least from 0º C to 100º C
?_________________________
6. What is the solubility of potassium nitrate at 90º C ?
______________________________________
7. At what temperature does potassium iodide have a solubility of 150 g/ 100 cm3 water
?________________________
8. You have a solution of sodium nitrate containing 140 g at 65º C. Is the solution
saturated, unsaturated, or supersaturated
?_____________________________________________________________
9. You have a solution of potassium chlorate containing 4 g at 65º C. How many
additional gramsof solute must be added to it, to make the solution saturated
?________________________________
10. A solution of potassium iodide at 70º C contains 200 g of dissolved solute in 100 cm3
water.
The solution is allowed to cool. At what new temperature would crystals begin to start
forming ?
Page 69 of 80
Chapter Fifteen
Acids and Bases
Page 70 of 80
Chapter Fifteen
Acids and Bases
Page 71 of 80
Chapter Fifteen
Acids and Bases
Page 72 of 80
Chapter Fifteen
Acids and Bases
Page 73 of 80
Chapter Fifteen
Acids and Bases
Chapter Fifteen
Acids and Bases
SECTION ONE: WHAT ARE ACIDS AND BASES? (pg. 530-538)
Conduct electricity
Have a conjugate
Have an Arhennius
definition
Have hydroxide ions
React with many
metals
Can be strong or
weak
Found in cleansers
Accept protons
Have a Bronsted
Lowry definition
Generate Hydronium
Ions
Donate protons
Found in fruit juice
Acid-Base Semantic Map
Acids
Bases
PRACTICE: WHAT IS AN ACID?
1. List two characteristics of acids and two characteristics of bases.
2. Complete the following: According to Arrhenius, all acids begin with a(n) ______________
and all bases contain a ________________.
3. A problem with the Arrhenius definition came about when scientists discovered that some
__________________ such as ammonia, did not contain the OH they expected.
4. Scientists _______________ and _________________ adjusted the definition of acids.
5. Acids are now considered proton _______________ and bases are proton ____________.
6. A proton is the same thing as a(n) _________________ ion.
7. Using the Arrhenius definition, label each of the following compounds: acid, base, neither.
e. Mg(OH)2
a. NaOH
b. HC2H3O2
f.
c. H3PO4
g. HCl
d. CaSO4
h. (NH4)2CO3
i.
LiOH
HI
Page 74 of 80
Chapter Fifteen
Acids and Bases
8. For the equations written below, you will identify the conjugate acid and base. Remember,
you will be labeling both sides. The first problem has been solved for you.
a. HC2H3O2 + CO32-  C2H3O1- + H2CO3
Acid
base
base
acid
b. HNO3 + NaOH  H2O + NaNO3
c. NH3 + H2O  NH4+ + OHd. HSO4- + HCN  H2SO4 + CNPRACTICE: WEAK AND STRONG ACIDS & BASES
Circle the correct word(s) to complete each statement.
1. A reaction is at equilibrium when the amounts of products and reactants are stable and
equal/unchanging.
2. In any acid equation, one of the products will always be H+/OH3. A strong acid is one in which most of the acid breaks apart/stays together.
4. Write equations showing the dissociation of each of the following acid and bases.
a. H2SO4
e. HF
b. NaOH
f.
c. HC2H3O2
g. Mg(OH)2
HI
d. Al(OH)3
Page 75 of 80
Chapter Fifteen
Acids and Bases
PRACTICE: pH WORKSHEET
Circle the correct word(s) to complete each statement.
1. Acids dissociate in water to produce hydroxide/hydronium ions.
2. The higher the hydronium concentration the more/less acidic a substance is.
3. A substance with a low pH will have a high/low hydronium ion concentration.
4. The pH scale is a measure of the hydronium/hydroxide ion concentration.
5. The pH scale goes from zero to fourteen/twenty, with six/seven representing neutral
and numbers above/below that representing acids.
6. Bases high on the pH scale are weaker/stronger than bases closer to neutral.
7. Acids low on the pH scale are weaker/stronger than acids closer to neutral.
8. A strong acid will conduct more/less than a weak acid due to the increase/decrease in
ions.
9. A weak base will conduct more/less than a strong base due to the increase/decrease
in ions.
10. Because H2SO4 is a strong acid/base, it will have a very high/low pH.
11. Vinegar has a [H3O+] of 1  10-6, which is higher/lower than milk’s [H3O+] of 1  10-8.
This means that vinegar is more/less acidic than milk.
12. For each of the common household compounds below, use their hydronium ion
concentration to calculate their pH.
a. Dill pickles
[H3O+] = 6.3  10-4
b. Cooked spinach
[H3O+] = 6.5  10-8
c. Milk of Magnesia
[H3O+] = 7.9  10-11
d. Cucumbers
[H3O+] = 7.9  10-6
e. Eggs
f. Battery Acid
[H3O+] = 5.01  10-9
[H3O+] = 1
g. Ammonia
[H3O+] = 3.16  10-12
h. Drain Cleaner
[H3O+] = 1  10-14
13. Draw a pH scale below and:
a. place the following terms on the scale: 0, 7, 14, neutral, acidic, basic.
b. draw arrows showing the direction(s) of increasing conductivity.
c. Place the items from #12 on the pH scale based on your calculated pH.
Page 76 of 80
Chapter Fifteen
Acids and Bases
14. Use your pH scale from #13 to answer the following:
a. What was the most acidic item on your #6 list?
b. What was the least acidic item?
c. What was the most basic?
d. Which item had the greatest hydronium ion concentration?
e. Which item has the lowest hydronium ion concentration?
Page 77 of 80
Chapter Fifteen
Acids and Bases
PRACTICE: NEUTRALIZATION WORKSHEET
Circle the word(s) which best complete each statement.
1. An acid has certain properties, such as reacting to metal, which are eliminated/enhanced
when the acid is neutralized.
2. In a neutralization reaction the products are always a(n) acid/water and a base/salt.
3. Scientists used indicators to determine the endpoint/concentration of a titration.
4. When neutralizing an acid, a more concentrated base will require a lower/higher volume
than one that is less concentrated.
5. Before performing titration calculations, it is necessary to know the concentration/volume
of your standard solution and the concentration/volume of your unknown solution.
6. The titration is completed to determine the volume/concentration of standard solution used,
which allows us to calculate the volume/concentration of the unknown solution.
7. Complete the following titration problems:
a. What volume of 3.5M NaOH will be required to titrate 100 ml of 3M HCl?
b. What volume of 1.2M KOH will be necessary to neutralize 750 ml of a 2.5M HNO 3
solution.
c. If I have 2.5L of Mg(OH)2, what concentration must it be to neutralize 330 ml of
1.2M HF?
d. Calculate the concentration of 200 ml of HCl necessary to neutralize 500 ml of
5.5M LiOH solution.
Page 78 of 80
Chapter Fifteen
Acids and Bases
Page 79 of 80
Chapter Fifteen
Acids and Bases
Page 80 of 80