2015-16 GenChem Final Review
Part I: MULTIPLE CHOICE QUESTIONS: 70% of Final
UNIT 7: 9.1 – 9.4
Stoichiometry
Consider the following equation for questions 1 thru 3
2C2H2 (g)+ 5O2 (g) → 4CO2 (g) + 2H2O(g)
acetylene
1) If 0.500 mol of acetylene is allowed to completely react with oxygen, what is the final yield of
CO2 in moles?
A) 2.00 mol
B) 4.00 mol
C) 1.00 mole
D) 0.100 mole
E) 0.500 mole
2) If 20.0 g of acetylene is allowed to completely react with oxygen, how many grams of O2 are
reacted?
A) 9.85 g
B) 24.6 g
C) 5.00 g
D) 61.4 g
E) 20.0 g
3) If 40.0 g of acetylene is allowed to react with 40.0 g of oxygen , how many grams of CO2 are
formed?
A) 135 g
B) 44.0 g
C) 40.0 g
D) 80.0 g
E) 55.0 g
4) When 50.0 g of acetylene is allowed to react with excess oxygen, 75.0 g of CO2 are formed.
What is the percent yield of carbon dioxide?
A) 100 %
B) 150 %
C) 6.7 %
D) 44.4 %
E) 88.8 %
5) Magnesium sulfate reacts with barium chloride according to the following balanced
equation. If 1.20 g of magnesium sulfate is allowed to react with 1.00 g of barium chloride in
a water solution, what is the limiting reagent?
MgSO4(aq) + BaCl2(aq) → BaSO4(s) + MgCl2(aq)
A)
B)
C)
D)
E)
magnesium chloride
barium chloride
magnesium sulfate
marium sulfate
water
UNIT 8: 3.3-3.5, 10.5
Thermochemistry
6) A solid is dissolved in a coffee cup calorimeter. Which of the following observations suggests that
the process is exothermic?
A) temperature of the solution decreases
B) temperature of the solution increases
C) temperature of the solution stays the same
7) The specific heat of a substance is defined as ___.
A) the energy required to raise the temperature of 1 gram of the substance by 1oC
B) the energy required to vaporize 1 mole of the substance at its normal boiling point
C) the average kinetic energy of the substance
D) the energy required to raise the temperature of the entire substance by 1o
E ) the hotness or coldness of the substance
8) The graph below represents the uniform heating of a solid, starting below its melting point.
What portion of the graph shows the warming of the liquid phase of the substance?
A) EF
B) AB
C) DE
D) CD
E) BC
9) What is the name of the process which occurs when a substance passes from the gas to the liquid
phase?
A) sublimation
B) condensation
C) melting D) freezing E) deposition
The following table lists the specific heats for a few substances. Use this table to answer Question 10 and 11
Substance
Copper (Cu)
Iron (Fe)
Silver (Ag)
Sodium chloride (NaCl)(s)
Ammonia (NH3)(g)
Specific Heat
(
)
0.385
0.452
0.235
0.864
2.04
10) If the same amount of heat is supplied to 10.0 g of each substance all at 21.0oC, which substance would
experience the LARGEST change in temperature?
A) Cu
B) Fe
C) Ag
D) NaCl
E) NH3
11) A 25.0 g piece of copper undergoes a temperature increase of 100.0oC. How much energy,
in joules, did the copper absorb ?
A) 962 J
B) 2500 J
C) 6490 J
D) 9.63 J
E) 0.0962 J
12) A solute is dissolved in water in a coffee cup calorimeter and the dissolving process results in a
positive ΔHSol'n. The temperature of the resulting solution will:
A) increase
B) decrease
C) stay the same
2
UNIT 9: Chp. 11.1-11.8, 11.10
Gas Laws
13) The “initial volume” balloon is at atmospheric pressure. Which balloon(s) shown above
represent the balloon after it has been put into a chamber with a lower pressure.
A) Balloon A
B ) Balloon B
C) Balloon C
D) Balloons B and C
E) Balloons A and B
14) Charles’s Law states that the volume of a gas _____ when the _____ decreases.
A)
B)
C)
D)
E)
increases, quantity of gas
decreases, temperature
decreases, pressure
increases, pressure
increases, temperature
15) What unit of temperature is used in gas law calculations?
A)
B)
C)
D)
E)
Kelvin
Celsius
Fahrenheit
either Celsius or Fahrenheit
either Celsius or Kelvin
16) 1 atmosphere of pressure is the same as ___ mmHg.
A) 1
B) 600
C) 200
D) 100
E) 760
17) According to the kinetic molecular, KMT, theory of gases, particles of a gas
A)
B)
C)
D)
E)
are very large
lose their valence electrons.
decrease in kinetic energy as temperature increases.
are very far apart.
move slowly.
18) According to Avogadro's law, the volume of a gas
A)
B)
C)
D)
E)
depends only on the number of moles in the sample.
is directly related to the number of moles at constant temperature and pressure.
is inversely related to the number of moles at standard temperature and pressure.
is inversely related to the number of moles at constant temperature and pressure.
depends only on the temperature and pressure.
3
19) At STP, temperature and pressure have the values of
A)
B)
C)
D)
E)
0 K and 1 atm.
760 K and 273 atm.
0 K and 760 mmHg.
273 K and 1 mmHg.
273 K and 760 mmHg.
20) The mathematical expression of the ideal gas law is ________.
A)
21)
𝑃1
𝑇1
=
𝑃2
B) PV = nRT
𝑇2
B) 12.2 L
B) 4120 L
D) 22.4 L
E) 44.0 L
C) 0.00600 L
D) 4.60 L
E) 5.40 L
C) 2.50 liters
D) 250. liters
E) 11.60 L
B) 1.1 atm
C) 0.47 atm
D) 0.47 atm
E) 0.94 atm
B) 690 mmHg
C) 470 mmHg
D) 210 mmHg
E) 1560 mmHg
The total pressure in a mixture of gases is equal to the partial pressure(s) of
the gas with the greatest number of moles.
all the gases added together.
the gas that occupies the largest volume.
the gas with the smallest number of moles.
the gas with the highest molecular weight.
A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of
cyclopropane in the mixture is 334 mmHg and the partial pressure of the oxygen is 1.02
atm, what is the total pressure of the mixture in torr?
A) 335 torr
28)
𝑉2
𝑃2
At 570. mmHg and 298 K a gas sample has a volume of 2270 mL. What is the final pressure
(in mmHg) at a volume of 1250 mL and a temperature of 448 K?
A)
B)
C)
D)
E)
27)
=
A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What
will be the gas pressure when the temperature changes to 450 K?
A) 7000 mmHg
26)
C) 273 L
B) 115 liters
A) 2.1 atm
25)
𝑉1
𝑃1
A 10.0 liter balloon was taken from a temperature of 298 K and placed in a freezer at a
temperature of 258 K. What was the new volume if pressure is constant?
A) 8.66 liters
24)
E)
The pressure of 5.00 L of gas increases from 1.50 atm to 1.63 atm. What is the final volume
of the gas, assuming constant temperature?
A) 5.00 L
23)
D) PT = P1 + P2 + P3….
At STP, what is the volume of 1.0 mol of carbon dioxide?
A) 1.00 L
22)
C) P1V1 = P2V2
B) 432 torr
C) 1.44 torr
D) 1110 torr
E) 760 torr
A 0.315 mol sample of He gas has a pressure of 0.123 atm at 428 Kelvin. What is the
volume of the sample?
A) 573 K
B) 546 L
C) 1.35 L
D) 118 L
E) 90.0 L
4
UNIT 10 : Chp. 9.5, 13.1-13.2, 13.5
Kinetics
For Questions 29-31, match the following to the energy diagram shown above.
29) activation energy, Ea
A) A
B) B
C) C
30) ΔHRXN
A) A
B) B
C) C
31) this reactions is
A) exothermic
B) endothermic
Answer Questions 32-35 based on the equilibrium equation shown below.
CO2 (g) + H2(g)
CO (g) + H2O(l)
ΔHRXN = ─ 2.8 kJ
In which direction will the equilibrium shift in response to each change listed below:
A) towards products
B) towards reactants
C) no change
Change
Direction of Shift
32)
33)
34)
35)
A)
A)
A)
A)
decrease temperature
decrease volume
add CO(g)
remove some H2O(l)
or
or
or
or
B)
B)
B)
B)
or
or
or
or
C)
C)
C)
C)
36) The following chemical equation represents what happens when solid NaOH heated.
NaOH(s) + HEAT → NaOH(l)
Which of the following phrases best describes this process?
A)
B)
C)
D)
E)
endothermic, heat is absorbed by the system
exothermic, heat is absorbed by the system
endothermic, heat is released by the system
exothermic, heat is released by the system
endothermic, heat is released by the surroundings
5
UNIT 11: 12.5
Solutions/ Dilutions
37) What volume of a 3.5 M stock solution is necessary to make 100. mL of a 0.1 M dilution?
A) 2.9 mL
B) 35 mL
C) 350 mL
D) 0.35 mL
E) 10. ml
38) What is the molarity of a solution which contains 58.4 g of sodium chloride dissolved in
500 mL of solution?
B) 1.00 M
C) 2.00 M
D) 0.500 M
E) 4.00 M
A) 1.50 M
39) How many moles of CaCl2 are in 150. mL of a 2.00 M of CaCl2 solution?
B) 0.300 mol C) 0.0133 mol D) 13.3 mol
E) 13.3 mol
A) 300. mol
40) How many milliliters of 2.25 M KOH solution are needed to provide 0.660 mol of KOH?
B) 2.93 mL
C) 293 mL
D) 29.3 mL
E) 34.1 mL
A) 0.293 mL
41) How many moles of CaCl2 are in 250. mL of a 3.00 M of CaCl2 solution?
A) 1.33 mol B) 0.750 mol
C) 83.3 mol
D) 750. mol E) 3.00 mole
42) What is the molarity of 500.0 mL of a dilution made with 50.0 mL of a 2.50 M stock solution?
A) 125 M
B) 1 × 104 M
C) 10 M
D) 20 M
E) 0.25 M
UNIT 12: Chp. 14.1,14.3, 14.5-14.8
Acids and Bases
43) The indicator phenolphthalein is ___ in acid and ___ in base.
A) colorless, pink
B) pink, blue
C) blue, pink
D) pink, colorless
E) light blue, dark blue
44) What type of reaction is shown by the chemical equation below?
HCl(aq) + NaOH(aq) → H2O(l)
A) single replacement
B) synthesis
C) neutralization
+ NaCl (aq)
D) combustion
45) What is the [OH - ] in a solution with [H3O+] = 1.0 × 10 − 10 M?
B) 1.0 × 10− 3 M
C) 1.0 × 102 M
D) 1.0 × 10− 4 M
A) 1.0 × 10− 7 M
46) Which of the following is incorrectly identified?
B) HF, strong acid
A) Ba(OH)2, strong base
C) NH3, weak base
E) 1.0 × 10− 18 M
D) HCl, strong acid
47) Calculate the acid concentration of a sample of acid rain with a pH of 8.11.
A) 4.2 × 10-1 M
B) 1.0 × 10-4 M
C) 0.62 M
D) 6.3 × 10-5 M
48) What is the pOH of a solution with a pH of 11.5?
A) 2.5
B) 0.115
C) 14.0
D) 0.25
E) decomposition
E) 7.7 × 10-9 M
E) 10.3
49) What is the pH of a solution with [H3O+ ] = 1.0 × 10− 5 M?
B) 5.0
C) -9.0
D) -5.0
E) 1.0 × 10− 5
A) 9.0
6
50) Which of the following is true in a acidic solution?
A) [H+] = [OH−]
B) [H+] > [OH−]
C) [H+] < [OH−]
D) [H+] = 0
E)
[OH−] = 0
51) A solution with a pH of 8.0 is ___ times more basic than a solution with a pH of 6.0
A) 1,000
B) 100
C) 10
D) 2
E) 0
52) The correct formula for hydrochloric acid is ___.
A) HClO3
B) HCl
C) HClO
D) HClO2
53) The correct name for H2CO3 is ___ acid.
A) carbonate
B) carbonous
C) hydrocarbonic
E)
H2Cl
D) carbonic
E) hydrogen carbide
54) Calculate the unknown concentration of H3PO4 if 50.0mL was titrated to the end point with 16.50 mL of a
2.0 M NaOH solution according to the following acid-base titration.
H3PO4 (aq) + 3 NaOH(aq) → 2 H2O(l)
A) 0.22 M
B)
0.033 M
C) 0.011 M
+ Na3PO4 (aq)
D) 11 M
E)
3M
55) What volume of 0.124 M KOH titrant was used to neutralize 23.4 mL of 0.206 M HCl solution?
A) 15.9 mL
B) 38.9 mL
C) 31.8 mL
D) 1.00 × 104 mL
E) 5.00 × 102 mL
UNIT 13: Chp. 10.1 – 10.4
Molecular Geometry and IMFs
56) Which of the following is the correct electron-dot structure for CS2?
A)
B)
C)
D)
E)
57) Which of the following substances contains a nonpolar bond?
A) N2
B) H2O
C) NH3
58) A polar covalent bond is found in which of these compounds?
A) H2O
B) F2
C) NaCl
D) NaCl
D) N2
E) MgF2
E) H2
59) The number of electron lone pairs in the water molecule is ________.
A) 3
B) 8
C) 1
D) 4
E) 2
60) If the electronegativity difference between elements X and Y is 2.1, the bond between the elements X-Y is ___.
A) ionic
b) impossible
C) metallic
D) nonpolar covalent
E) polar covalent
61)
7
The
VSEPR theory allows us to determine the ________.
A) color of a compound
B) formula for a compound
C) shape of a molecule
D) bond type for a molecule
E) charge on an ion
62) The molecular shape of the ammonia molecule, NH3, is ___.
A) trigonal pyramidal
B) linear
C) octagonal
D) square
E) hexagonal
63) The water molecule has a molecular dipole with the negative portion
A) localized between the hydrogen atoms.
B) surrounding the molecule.
C) localized on one of the hydrogens.
D) pointing toward the oxygen atom.
E) pointing from the oxygen through the hydrogen atoms.
64) The carbon tetrachloride molecule, CCl 4, has the shape of a ________.
C) tetrahedron
A) square
B) cube
D) sphere
E) circle
65) The bond dipole in the nitrogen-hydrogen bond points
A) from the nitrogen to the hydrogen.
B) at the observer.
C) at right angles to the bond.
D) in a circle surrounding the bond.
E) from the hydrogen to the nitrogen.
66) The Lewis structures for methanol and ethanol are shown below. The difference in boiling point is
most due to ___.
ethanol:
boiling point = 78oC
methanol:
boiling point = 65oC
A)
B)
C)
D)
E)
dipole-dipole interactions
hydrogen bonding
London dispersion forces
Ion-dipole interacdtions
Metallic bonding
67) The main interactions between molecules of methane, CH4, are ________.
A) dispersion forces
B) dipole-dipole attractions
C) ionic bonds
D) hydrogen bonds
E) none of the above
END
8
2015-16 GenChem Final Review
Equations:
Equations/ Constants
Constants
q = mSHΔT
KW = [H3O+][OH−]
KW = 1.0 x 10−14
14 = pH + pOH
Avogadro's Number 6.022 x 1023
pH = − log [H3O+]
pOH = − log [OH−]
𝟎.𝟎𝟖𝟐𝟏 𝒂𝒕𝒎 ∙𝑳
R=
𝒎𝒐𝒍 ∙𝑲
M1V1 = M2V2
Molarity (M) =
𝑽𝟏
𝑻𝟏
=
𝐦𝐨𝐥𝐞𝐬 𝐬𝐨𝐥𝐮𝐭𝐞
𝐥𝐢𝐭𝐞𝐫𝐬 𝐬𝐨𝐥𝐮𝐭𝐢𝐨𝐧
𝑽𝟐
𝒈 • 𝑪𝒐
1 atmosphere
1 atm
760 millimeters of mercury
760 mmHg
PT = P1 + P2 + P3...
29.9 inches of mercury
29.9 in Hg
𝑽𝟏 𝑷𝟏
760 torricelli
760 torr
101,325 Pascal
101,325 Pa
PV = nRT
101.325 kilopascal
101.325 kPa
𝑽𝟏
14.70 pounds per square inch
14.70 lb/ in2
𝒏𝟏
𝑷𝟏
𝑻𝟏
𝑽𝟐 𝑷𝟐
=
𝑻𝟏
𝑻𝟐
=
𝑽𝟐
=
𝑷𝟐
𝒏𝟐
𝑻𝟐
A = Central Atom
Electron
Groups
𝟒.𝟏𝟖𝟒 𝑱
Standard Atmospheric Pressure Units:
𝑻𝟐
V1P1 = V2P2
KEY:
S𝑯𝑯𝟐 𝑶 =
X = bonded atom
E = lone pair of electrons
Molecular Geometry Name
1
lone pair
2
lone pair
3
lone pair
5
See-Saw
4 bonds
T-Shaped 3 bonds
Linear
2 bonds
6
Square Pyramidal 5 bonds
Square Planar
4 bonds
9
Solubility Rules
Soluble Compounds










all ammonium (NH4+) compounds
all Group I compounds
all nitrates (NO3─) compounds
all acetate (CH3COO─) compounds
all chlorate (ClO3─) compounds
all perchlorates (ClO4─)
chlorides - except Ag+ Pb2+ , Hg22+
bromides - except Ag+ Pb2+ , Hg22+
iodides - except Ag+ Pb2+ , Hg22+
sulfates (SO42─) - except Ag+, Pb2+ , Ba2+, Sr2+, Ca2+
Insoluble Compounds




sulfides – except Ba2+, Ca2+, Sr2+
carbonates (CO32─)
phosphates (PO43─)
hydroxides (OH─) – except Ba2+, Ca2+, Sr2+
10
11
2015/16 GenChem Final Review
Part II: EXTENDED RESPONSE QUESTIONS:
30% of Final
Unit 7: Stoichiometry
1.
Use the following reaction to answer Questions 9 thru 11. For ALL questions, show ALL your work and
circle your final answers. Be sure to include units with your answers.
Mg3N2(s) + 6 H2O (l) → 3 Mg(OH)2(s) + 2 NH3(g)
A. What is the limiting reactant of the above reaction if 20 g of Mg3N2 is reacted with 25 g of water?
𝟏 𝒎𝒐𝒍 𝑴𝒈𝟑 𝑵𝟐
×
20 g Mg3N2
𝟏𝟎𝟎.𝟗𝟓 𝒈
×
𝟐 𝒎𝒐𝒍 𝑵𝑯𝟑
𝟏 𝒎𝒐𝒍 𝑴𝒈𝟑 𝑵𝟐
= 0.40 mol NH3
Mg3N2 is limiting
25 g H2O
×
𝟏 𝒎𝒐𝒍 𝑯𝟐 𝑶
𝟏𝟖.𝟎𝟐 𝒈
×
𝟐 𝒎𝒐𝒍 𝑵𝑯𝟑
𝟔 𝒎𝒐𝒍 𝑯𝟐 𝑶
= 0.69 mol NH3
B. What is the theoretical yield, in grams, of ammonia, NH3?
0.40 mol NH3
×
𝟏𝟕.𝟎𝟒 𝒈 𝑵𝑯𝟑
𝟏 𝒎𝒐𝒍 𝑵𝑯𝟑
=
6.8 g
NH3
C. If the actual yield of ammonia was 6.5 grams, what is the percent yield of this reaction?
𝟔.𝟓 𝒈 𝒂𝒄𝒕𝒖𝒂𝒍 𝒚𝒊𝒆𝒍𝒅
𝟔.𝟖 𝒈 𝒕𝒉𝒆𝒐𝒓𝒆𝒕𝒊𝒄𝒂𝒍 𝒚𝒊𝒆𝒍𝒅
×
100 =
96% yield
12
Unit 8: Thermochemistry
2. A 50.0 g of calcium chloride were dissolved in 200.0 mL of distilled water in a coffee-cup calorimeter
according to the following equation:
CaCl2(s)
→
Ca2+(aq)
+
2Cl – (aq)
ΔHSol’n =
– 82.9+ kJ/ mol
(a) Was the dissolving of CaCl2 an exothermic or endothermic process? Explain.
exothermic, because ΔHSol’n for the process was negative.
(b) If the temperature of the water in the coffee-cup calorimeter increased, did the chemicals release or
absorb energy during the dissolving process? Justify your answer.
chemicals = released energy
the water absorbed the energy – this is what caused the
temperature of the water to increase
(c) Calculate the amount of energychange caused when the 50.0 grams of calcium chloride dissolved.
Show ALL work, circle final answer. Include units.
first: use molar mass to calculate the moles of CaCl2
50.0 g CaCl2
×
𝟏 𝒎𝒐𝒍𝒆
𝟏𝟏𝟎.𝟗𝟖 𝒈
=
0.451 mol
second: use ΔHSol’n to calcualte the enrgy released
0.451 mol
×
− 𝟖𝟐.𝟗 𝒌𝑱
𝒎𝒐𝒍
=
– 37.4 kJ
(d) Calculate the change in temperature, in oC, of the water. Show ALL work, circle final answer.
first: turn kilojoules into joules
– 37.4 kJ = – 37,400 J
second: use q = mSHΔT to calcualte ΔT
q = mSHΔT → 37,400 J = 250.0 g (=
𝟒.𝟏𝟖𝟒 𝑱
𝒈 • 𝑪𝒐
)ΔT = 35.8 oC
13
Unit 9: Gas Laws
Use the above table of Vapor Pressure of Water to help answer question 7.
3. A 550-mL sample of hydrogen gas (H2) was collected over water at an atmospheric pressure of 105.7 kPa and
a temperature of 50.0oC.
(a) Calculate the partial pressure, in kPa of hydrogen gas. Follow ALL math work rules!
PT = 𝑷𝑯𝟐 + 𝑷𝑯𝟐 𝑶 → 105.7 kPa = 𝑷𝑯𝟐 + 12.3 kPa
→ 𝑷𝑯𝟐 = 105.7 kPa – 12.3 kPa → 𝑷𝑯𝟐 = 93.4 kPa
(b) Convert the answer from (a) to pressure units of atmospheres. Follow ALL math work rules!
93.4 kPa ×
𝟏 𝒂𝒕𝒏
𝟏𝟎𝟏.𝟑 𝒌𝑷𝒂
= 0.922 atm
(c) Calculate the number of moles of hydrogen gas collected. Follow ALL math work rules!
PV = nRT → (0.922 atm)(0.550 L) = n (
𝟎.𝟎𝟖𝟐𝟏 𝐚𝐭𝐦 ∙𝐋
𝐦𝐨𝐥 ∙𝐊
)(323 K)
→ n = 0.0191 mol H2
14
Unit 11: Solutions
For the following questions assume that the only materials available to you are those in the
Materials List shown above.
4.
(a) You have been asked by your teacher to make 100-mL of a 0.35 M solution of NaCl starting
with solid NaCl.
(i)
List any mathematical calculations you would need to make before you could start to make
this solution.
 moles of NaCl required, and
 grams of NaCl required
(ii) Complete the calculation(s) from step 3(a)(i)
0.35 M is the same as
….
𝟎.𝟑𝟓 𝒎𝒐𝒍𝒆𝒔 𝑪𝒂𝑪𝒍𝟐
𝟏 𝒍𝒊𝒕𝒆𝒓
𝟎.𝟑𝟓 𝒎𝒐𝒍𝒆𝒔 𝑵𝒂𝑪𝒍
𝟏 𝒍𝒊𝒕𝒆𝒓
, so……
× 0.100 L = 0.035 moles NaCl required
NaCl = 58.44 g/ mol, so…..
... 0.035 mol NaCl ×
𝟓𝟖.𝟒𝟒 𝒈 𝑵𝒂𝑪𝒍
𝟏 𝒎𝒐𝒍𝒆
= 2.0 grams of NaCl required
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4. Continued:
(b) Explain how you would prepare this solution. The following lab equipment is available to you.
Clearly identify the equipment and size being used.
Materials List:






100-mL burette
100-mL beaker
100-mL Erlenmeyer flask
100-mL graduated cylinder
100-mL volumetric flask
2-mL disposal pipettes






chemical scoop
distilled water
tap water
electronic balance
glass stirring rod
hot plate w/ stir function





iron ring
lab goggles and gloves
powder funnel
ring stands and clamp
weigh boat
Write your procedure in bulleted form – failure to do so will result in a substantial loss of points.
 Mass out 2.0 grams of NaCl using a chemical scoop, weigh
boat, and electronic gram balance
 Use a powder funnel to transfer the NaCl to a 100-mL
volumetric flask
 Add distilled water to the volumetric flask until it is about
half full.
 Vigorously swirl the volumetric flask until the NaCl is
completely dissolved.

Fill the volumetric flask with distilled water until the bottom
of the meniscus is even with the fill line on the flask
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Unit 12: Acids and Bases
5.
neutralization
(a) The reaction that occurs between and acid and a base is called a(n) ____________________
reaction.
and salt
(b) What products are always formed when an acid and a base react? water
____________________
(c)
Write the balanced chemical equation for the reaction between solid lead (II) hydroxide
and sulfuric acid. Be sure to include all phases of mater.
Pb(OH)2(s)
+
H2SO4(aq)
→
PbSO4(s)
+
2 H2O(l)
Unit 13: Molecular Geometry and IMFs
6. Below is the Lewis structure for BrF4.
= individual bond dipoles
octahedral
(a) Name the electron pair (group) geometry: _____________________________
octahedral
(b) Name the molecular geometry: _______________________________________
(c) Draw in ALL bond dipoles.
(d) Does this molecule have a molecular dipole? If YES, use an arrow to draw in the molecular
dipole and then use the appropriate symbols to indicate the areas of partial positive and
negative charge (if any.) If NO, explain why not.
This molecule does NOT have a molecular dipole. The individual
bond dipoles are symmetrical and of equal magnitude and so they
“cancel out”.
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