Spring 2-14 Chemistry Review Material
Acids, Bases, and Salts
Name______________



An Arrhenius acid is defined as any compound that dissociates in aqueous solution to form
____________ ions.
HNO3 H+ + NO3
HCl (aq)  ________________________
An Arrhenius base is defined as any compound that dissociates in aqueous solution to form
____________ ions.
KOH (aq) K+ (aq) + OH- (aq)
NaOH (aq) ________________________
Salts are compounds that dissociate in aqueous solution releasing neither ____________ ions nor
____________ ions.
KCl (aq)  K+ (aq) + Cl- (aq)
NaCl (aq)  ________________________
Using the Arrhenius definition, classify the following examples as acids, bases, or salts:
HBr ____________________
KCl __________________
Mg(OH)2 ________________
H3PO4 ________________
HCl ____________________
HClO _________________
KNO2 ___________________
Al(OH)3 ________________
HFO4 ___________________
KC2H3O2 _______________
Ba(OH)2 _________________
NaCl __________________
Acids and bases can also be identified using an operational definition. Operational definitions are simply a list
of properties.
ACIDS:
♦ A ____________ taste is a characteristic property of all acids in aqueous solution.
♦ Acids react with some metals to produce ____________ gas.
♦ Because aqueous acid solutions conduct electricity, they are identified as ____________.
♦ Acids react with bases to produce a ____________ and water.
♦ Acids turn ____________ different colors.
BASES:
♦ Bases tend to taste ____________ and feel ____________.
♦ Like acids, aqueous basic solutions conduct ____________, and are identified as
____________.
♦ Bases react with ____________ to produce a salt and ____________.
♦ Bases turn ____________ different colors.
Naming Acids


Binary acids consist of ____________ elements, the first being ____________.
Ternary acids consist of ____________ elements. Do NOT use a prefix.
–ate becomes _______ and –ite becomes _______
Give the word equation for the neutralization reaction of an acid and a base.
Answer questions and problems on your own paper.
Spring 2-14 Chemistry Review Material
Chemical Quantities Worksheet
Name ______________________________
Period _____ Date ___________________
Recipes often specify the number of
eggs needed. Although eggs are used
individually when cooking small
quantities, they are sold by the dozen,
or by the gross (144, a dozen dozens),
depending on the quantity wanted. If
you were cooking for an army, you'd
likely mix your eggs by the gross,
rather than counting them individually.
Instead of thinking in terms of 2 eggs
per potato, you'd use 2 gross of eggs
per gross of potatoes.
If you were buying rice for a casserole,
would you go to a store and ask for
250,000 rice grains? Or would you
ask for a pound of rice? Because rice
is small, it's convenient to use other
means of measuring than counting.
Chemical particles (atoms, molecules,
etc.) are much, much, smaller than
eggs or rice. It is therefore more
convenient and useful to specify
quantities in ways other than by
counting individual atoms or
molecules. The quantity called the
mole is used to specify the number of
Answer questions and problems on your own paper.
particles, just like the dozen or gross is
used for eggs and other items we
encounter in our daily lives. Whereas
a dozen is 12 of something, and a gross
is 144 of something, a mole is 6.02 x
1023 of something
(602,000,000,000,000,000,000,000).
If a chemical reaction involves one
atom of magnesium and two units of
hydrochloric acid, one mole of
magnesium will react with two moles
of hydrochloric acid. We can't pick
out individual chemical particles, but
we can easily measure a mole of them.
How do we measure moles? We use a
balance to determine the mass, and
then convert mass to moles. Just as the
mass of a gross of eggs differs from
the mass of a gross of potatoes, the
mass of a mole of aluminum atoms
differs from the mass of a mole of
calcium. The periodic table tells us the
mass of one mole of each element. For
instance, a mole of aluminum has a
mass of 26.98 grams. A mole of
calcium has a mass of 40.08 grams.
Spring 2-14 Chemistry Review Material
Use the periodic table to determine the mass of the following quantities of chemical
substances. Remember, the periodic table tells you the MOLAR MASS, the mass of one mole of
each element. The mass of two moles would be twice that of one mole. For compounds, add
the molar masses in the ratios indicated in the chemical formulas for the molar mass of the
compound.
1 mole of lithium
_______________
1 mole of hydrogen
_______________
1 mole of magnesium
_______________
2 moles of hydrogen
_______________
1 mole of carbon
_______________
1 mole of H2O
_______________
1 mole of oxygen
_______________
1 mole of CO2
_______________
2 moles of oxygen
_______________
2 moles of CO2
_______________
Use the periodic table to determine the number of moles in the following masses. Remember,
the periodic table tells you the MOLAR MASS, the mass of one mole of each element. For
compounds, add the molar masses in the ratios indicated in the chemical formulas for the mass
of one MOLE of the COMPOUND. Divide the mass indicated by the molar mass to calculate
the number of moles.
Answer questions and problems on your own paper.
Spring 2-14 Chemistry Review Material
35.45 grams of chlorine _______________
63.55 grams of copper
_______________
18.024 g of beryllium
_______________
36.033 grams of carbon _______________
100 grams of hydrogen _______________
100 grams of iron
_______________
100 grams of lead
_______________
18.0 grams of H2O
_______________
36.0 grams of H2O
_______________
100 grams of H2O
_______________
1. Balance the following equation: ____ K2PtCl4 + ___ NH3 → ___ Pt(NH3)2Cl2 +___ KCl
Determine the grams of KCl produced (theoretical yield) if you start with 34.5 grams of NH3.
2. Balance the following equation: H3PO4 + 3 KOH → K3PO4 + 3 H2O
If 49.0 g of H3PO4 reacts, how many grams of K3PO4 should be produced?
3. Balance the following equation: Al2(SO3)3 + 6 NaOH → 3 Na2SO3 + 2 Al(OH)3
If you start with 389.4 g of Al2(SO3)3 and how many grams of Na2SO3 would be produced?
4. Balance the following equation: Al(OH)3 (s) + 3 HCl (aq) → AlCl3 (aq) + 3 H2O (l)
If you start with 50.3 g of Al(OH)3 how many grams of AlCl3 would you expect to produce?
Assume you did the experiment and you only got 39.5 g of AlCl3, what is the percent yield
(hint: think about how you determine your % for a test – what you got divided by what you
should have gotten)?
Complete on our own paper.
Spring 2-14 Chemistry Review Material
5. Balance the following equation: K2CO3 + 2 HCl → H2O + CO2 + 2 KCl
Determine the theoretical yield (grams) of H2O if you start with 34.5 g of K2CO3. If only 3.4 g
of H2O is produced, what is the percent yield?
6. Balance the following equation: H2SO4 + Ba(OH)2 → BaSO4 + 2 H2O
a) If 98.0 g of H2SO4 reacts, how many grams of BaSO4 should be produced? b) What
is the percent yield if you only produce 213.7 g of BaSO4? (use the answer from a to
determine the answer for b)
Gas Laws
SHOW ALL WORK FOR ALL PROBLEMS
I. 1.0 atm = 101.3 kPa = 760 mmHg And 0C = 273 K
Change the following units:
359 kPa = _________ atm
10C = ________ K
6.2 atm = ________ kPa 10K = _______ C
For the rest of the problems: First identify each number with P, V, or T. Second state whose
law you are using, Third – show the equation, Fourth solve the problem, and Fifth - circle
your final answer - and make sure you don't forget your units!!!
1. The gas in a sealed can is at a pressure of 3.00 atm at 25C. A warning on the can tells
the user not to store the can in a place where the temperature will exceed 52C. What
would the gas pressure in the can be at 52C?
2. A sample of hydrogen exerts a pressure of 0.329 atm at 47C. The gas is heated 77C at
constant volume. What will its new pressure be?
3. 3. A sample of neon gas occupies a volume of 752 mL at 25C. What volume will the
gas occupy at standard temperature if the pressure remains constant?
4. A sample of oxygen gas has a volume of 150 mL when its pressure is 440 mmHg. If the
pressure is increased to standard pressure and the temperature remains constant, what will
the new gas volume be?
5. Ral3ph had a helium balloon with a volume of 4.88 liters at 150 kPa of pressure. If the
volume is changed to 3.15 liters, what would be the new pressure in atm?
Complete on our own paper.
Spring 2-14 Chemistry Review Material
6. 5.36 liters of nitrogen gas are at -25C and 733 mm Hg. What would be the volume at 128C
and 1.5atm?
7. At constant temperature, 2 L of a gas at 4 atm of pressure is expanded to 6 L. What is the
new pressure? (Do this one conceptually and not algebraically.)
Thermochemistry
Specific Heat Worksheet
C = q/m∆T, where q = heat energy, m = mass, and T = temperature Remember, ∆T =
(Tfinal – Tinitial). Show all work and proper units.
1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature
changes from 25°C to 175°C. Calculate the specific heat capacity of iron.
2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum
from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C?
3. To what temperature will a 50.0 g piece of glass raise if it absorbs 5275 joules of heat
and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is
20.0°C.
4. Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs
6.75×104 joules of heat, and its temperature changes from 32°C to 57°C.
5. 100.0 mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of
water is 4.18 J/g°C, calculate the amount of heat energy needed to cause this rise in
temperature.
What is enthalpy?
What is enthalpy?
What is Hess’s Law?
Complete on our own paper.
Spring 2-14 Chemistry Review Material
Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
PCl5(g) → PCl3(g) + Cl2(g)
P4(s) + 6Cl2(g) → 4PCl3(g)
4PCl5(g) → P4(s) + 10Cl 2(g)
ΔH = -2439 kJ
ΔH = 3438 kJ
(2) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
2CO2(g) + H2O(g) → C 2H2(g) + 5/2O2(g)
C2H2(g) + 2H2(g) → C2H6(g)
H2O(g) → H2(g) + 1/2O2 (g)
C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g)
ΔH =-94.5 kJ
ΔH =71.2 kJ
ΔH =-283 kJ
3) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
N2H4(l) + H2(g) → 2NH3(g)
N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g)
N2(g) + 3H2(g) → 2NH 3(g)
CH4O(l) → CH2O(g) + H 2(g)
ΔH = -37 kJ
ΔH = -46 kJ
ΔH = -65 kJ
(4) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
H2SO4(l) → SO3(g) + H2O(g)
H2S(g) + 2O2(g) → H2SO4(l)
H2S(g) + 2O2(g) → SO 3(g) + H2O(l)
H2O(l) → H2O(g)
ΔH = -235.5 kJ
ΔH = -207 kJ
ΔH = 44 kJ
(5) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
2C2H4O(l) + 2H2O(l) → 2C2H6O(l) + O2(g)
C2H6O(l) + 3O2(g) → 2CO2(g) + 3H2O(l)
C2H4O(l) + 5/2O2(g) → 2CO2(g) + 2H2O(l)
Nuclear Chemistry
What is nuclear fission?
What is nuclear Fusion?
Where is Nuclear Fusion used?
What are Isotopes?
What is a chain reaction?
Write the equations for:
1) the alpha decay of radon198
Complete on our own paper.
ΔH = -685.5 kJ
ΔH = -583.5 kJ
Spring 2-14 Chemistry Review Material
2) The beta decay of uranium 237
3) Positron emission from sodium 22
4) Write the symbols for an alpha particle, beta particle, gamma ray, and
positron.
5) If the half-life for the radioactive decay of Mendelevium 101 is 5 minutes and I
start with a 130 gram sample, how much will be left over after 60 minutes?
Complete on our own paper.
Spring 2-14 Chemistry Review Material
Chemistry Semester Two Key Term List
These are the terms you are expected to know the meaning of when read, by the time you have
completed Spring Chemistry.
Molarity
solute
Solvent
boiling point elevation Brownian motion
colligative property
concentration
dilution
freezing point depression
heat of solution
hydrogen bonding
immiscible
insoluble
miscible
osmotic pressure
osmosis
saturated
solubility
solution
supersaturated
unsaturated
amphoteric
neutralization
Acid
Anhydride
Arrhenius acid/base
Base
Bronsted-Lowry model buffer
conjugate acid/base
equivalence point
Hydronium ion
Indicator
Ionization
pH, pOH
salt
standard solution
strong acid/base
titration
weak acid/base
Ka and Kb
Lewis acid/base
Kelvin
Standard pressure
Standard temperature
atmospheric pressure
Avogadro’s principle
Barometer
Boyle’s Law
Charles’s Law
Combined Gas Law
Gay-Lussac’s Law
Ideal Gas Law
Kinetic molecular theory
Pascal
enthalpy
specific heat
activated complex
activation energy
calorie
catalyst
collision theory
energy
entropy
heat
heat of formation
heat of reaction
inhibitor
intermediate
Joule
law of conservation of energy
reaction rate
spontaneous process
thermochemical equation chemical potential energy
Gibbs Free Energy
spontaneous reaction state functions
fission
fusion
alpha particle
atom
atomic mass
atomic mass unit
atomic number
beta particle
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Spring 2-14 Chemistry Review Material
chain reaction
electron
gamma radiation
half-life
isotope
mass number
neutron
nuclear reaction
nucleus
positron
proton
radiation
radioactive decay
Functional group
Organic molecule
Alcohols
Aldehydes
Alkane
Alkene
Alkyl Halides
Alkyne
Amines
Aromatic
Carboxylic acids
Cycloalkanes
Esters
Ethers
Geometric isomers
Ketones
Monomer
Polymer
Saturated hydrocarbons Structural isomers
Unsaturated hydrocarbon
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