Class _ __
Date ~ ~e.b } .u
Mixed Compounds
Name.
Write formulas.
1. so3
71.
2. KCl
22. sulfur hexafluoride
3. MgS0 4
23. iron(II) oxide
4. P20s
24. lithium iodide
5. CuCl
25. sodium bicarbonate
6. CuCh
26. strontium nitrate
7. AgN03
27. ammonium chloride
8. CaC03
28 . diarsenic trioxide
9. Ca(OH)2
29. copper(II) sulfate
10. Fe203
30. aluminum oxide
11. BaS04
31. mercury(II) sulfite
12. CuS
32. dinitrogen tetroxide
13. KMn0 4
33. potassium acetate
14. LiHC03
34. tin(IT) fluoride
15. SnF4
35. potassium hydroxide
16. CN'H4)2S04 -
-
- -- -- -- -
sodium chloride
36. lead(II) chloride
17. Na3P04
37. chromium(III) bromide
18. ZnO
38. silicon dioxide
19. CC4
39. iron(II) phosphate
20. Ca(N03)2
40. nickel(IT) nitrite
41. Differentiate between S03 and SO/.
42. A molecular compound is formed when - - -- -- - - -- - -- - - combine.
43. An ionic compound is formed when a _ __ _ __ __ and a _ _ _ _ _ _ _ _ combine.
44. The smallest particle of a molecular compound that has the properties of the compound is a
45. The smallest unit of an ionic compound is a _ __ __ _ _ _
Nrume _________ ________ ________ ________ ____
Class _ _ _
Date - --- - -
Balancing Word Equations
Write the word equations below as chemical equations and balance.
1. zinc + lead(II) nitrate -+ zinc nitrate + lead
2. aluminum bromide and chlorine form aluminum chloride and bromine
3. sodium phosphate plus calcium chloride produce calcium phosphate plus sodium chloride
4. potassium chlorate when heated yields potassium chloride and oxygen gas
Balance the chemical equations below and write word equations for each.
5.
AI
+
7.
8. __ H2 +
HCI
-+
AICh
+ · __ H2 (gJ
Nrume ___________________________________
Class - --
Date--~----
Molecular Geometry
For each of the following molecules: (1) draw the Lewis Structure, (2) use VSEPR theory to determine
the shape and bond angle, (3) sketch the molecule and label each dipole moment(~). and (4) state
whether the molecule is polar or nonpolar.
Molecule
1. AsH3
2.BF3
3. BeBr2
4.SCh
S.CHCh
Lewis Structure
Molecular Shape
& Bond Angle
Sketch
Molecular
Polarity
Molecule
6. PFs
7. SF6
Lewis Structure
Molecular Shape
& Bond Angle
Sketch
Molecular
Polarity
Nrune ____________________________________
Class ______
Date ___ _ _ __
Stoichiometric Calculations
1. How many moles of KCI0 3 must decompose in order to produce 9 moles of oxygen gas?
2KC103(s)
~
2KCl(s) + 30 2(g)
2. How many grruns of KC10 3 are required to produce 7.50 moles of KCI?
2KCIOJ(s) ~ 2KCI(s) + 302(g)
3. How many moles of water are produced from 58 g of oxygen gas?
__ H2+ __ 02~ __ H20
4. How many grams of hydrogen gas would be needed to form 8.0 grams of water?
__ H2 + __ 02
~
__ H20
5. How many grams of silver will be formed from 12.0 g magnesium?
_
Mg(s) + _
AgN03(aq) ~ _
Ag(s) + _
Mg(N0 3)2(aq)
6. Iron reacts with chlorine gas to form iron(III) chloride. How many grams of iron(III) chloride are
formed from 112 g of iron? (First, write the balanced equation.)
·:~
-~~~ ~- ---:":"'"·"..;..~
-.- .
7. Calculate the number of grams of nitrogen gas required to make 1.22 L of ammonia at STP.
_ _ N2+ _ _ H2~ _ _ NH3
8. How many grams of zinc are required to react with 125 mL of3.00Mhydrochloric acid?
_ _ Zn + _ _ HCI
~
__ ZnCh + _ _ H 2
9. How many liters of hydrogen gas will be produced by 5.6 g of zinc at STP?
_ _ Zn+ _ _ HCI~ _ _ ZnCh+ _ _ H2
10. What volume of0.50M AgN03 is required to react with 25.0 L of l.SMCaCh? (First, write a
balanced equation.)
_ _ AgN0 3 + _ _ CaCh ~ _ _ AgCI + _ _ Ca(N03) 2
Nrune _____________________________________
Class ____
Date-----=------ -
Limiting Reactants & Percent Yield
1. When 16.3 g of magnesium and 45.2 g of oxygen gas react, how many grruns of magnesium oxide
will be formed? Identify the limiting and excess reactants.
2 Mg + 0 2 --)- 2 MgO
2. If2.45 g of iron are placed in 1.5 L of0.25M HCl, how many grams ofFeC12 are obtained? Identify
the limiting and excess reactants in this single replacement reaction.
Fe+ 2 HCl --)- FeCh + H2
3. Identify the limiting and excess reagents when 25 L of nitrogen reacts with 25 L ofhydrogen at STP.
How many liters of ammonia gas are formed in this reaction?
·
__ N2 + __ H2--)- __ NH3
4. 50.0 mL of2.00MH2S04 react with 75.0 mL of2.00MNaOH. Identify the limiting and excess
reactants. How many grams ofNa2S04 will be formed?
_ _ H2 S04 + __ NaOH--)- _ _ Na2S0 4 + __ H20
5. A chemist burns 16.0 g of aluminum in 50.0 L of oxygen to produce aluminum oxide at STP. First,
write a balanced equation. Then, identify the limiting and excess reactants and calculate the grams of
aluminum oxide formed.
6. If6.57 g of iron are reacted with an excess of hydrochloric acid, HCI, then hydrogen gas and 17.63 g
of iron(III) chloride are obtained. Calculate the theoretical yield and percent yield of FeCh.
_ _ Fe+ _ _ HCJ-+ _ _ H2 + _ _ FeCh
7. You need to produce 100.0 g ofFeCb in the following reaction. If the percent yield ofthe reaction
was 85.0%, how many grams of iron would you need to start with?
_ _ Fe+ _ _ HCI ~ _ _ H2 + - -. FeCh
_,
Name _____________________________________
:- -
. --~-~--~-- 7.~~:-~'.:-:~o
.--~:
-~ _:~-:::· - '
Class _ _ __
Date ___________
Calculating Molarity by Mass
Background
Water is such a common substance that chemical reactions often take place in solution. The
concentration of solutions can qualitatively be described as dilute or concentrated. Quantitatively the
concentration of solutions is most often measured in molarity (M) expressed in moles of solute/liter of
solution. Perform the following calculations. Show work. Label and round numbers appropriately.
Calculations
1. If a solution contains 3.458 moles ofCuCI2
in 1.500 L, what is the solution's molarity?
2. How many moles of LiN03 are in 250. mL
of 0.30M solution?
3. A solution is made by dissolving 95.7 g
NaOH to make 1.00 L solution. What is
the concentration ofthe solution?
4. How many grams KI are needed to prepare
100. mL of 0.55M solution?
5. What is the molarity of a sodium chloride
solution made by dissolving 263.7 g to make
2.0 L?
6. What mass CaBr2 is needed to make 500.0
mL of 0.554M solution?
Nrume _____________________________________
Class _ __
Date --- - ----
Calculating Molarity by Dilution
Background
Concentrated solutions can be purchased, then diluted to inake the concentration needed. In dilution,
only solvent is added, not solute. The number of moles of solute is the same before and after the dilution,
only the volume of the solution is changed. The measurements of the original solution have"!"
subscripts; the new solution has " 2" subscripts. moles 1 = moles 2 We can calculate the number of
moles in a solution by multiplying M 1V1 = M2V2. Use this equation to solve the following dilution
problems. Show work using dimensional analysis.
Calculations
1. Concentrated HCl is 11. 7M. What is the
concentration of a solution made by diluting
25.0 mL to 1000. mL?
2. What volume of 15.6M N}-40H is needed
to make 500. mL of 3 .OOM solution?
3. What volume of0.085M H2 S04 can be prepared
from 15.0 mL of 35.9M sulfuric acid?
4. A solution was prepared by diluting 50.00
mL to 250. mL of0.477M KOH. What was
the concentration of the original solution?
5. 2.0 L ofHC2H30 2 (acetic acid) is made by
diluting 75. mL of 17.6M acetic acid.
What is the molarity of the new solution?
6.
What volume of 6.5 8M HCI (hydrochloric
acid) is needed to make 500. mL of3.00M
HCI?
Nmne _____________________________________
Class ______
Date ----------
pH Calculations
Definition
The pH of an aqueous solution is mathematically defined to the right. For
integer values of the exponent on 10, pH can be found by inspection. For
non-integer values, pH can be found using the log function. (H30+ represents
the hydrated hydrogen ion.)
Calculating pH
Determine the pH for each [H30j below.
1 X 10"2M
2.
3.
6.75
X
10"2 M
Cal~ulate the [H30j for the given pH values below. (Use the antilog or log" 1 function on your calculator.)
_ _ _ _ _ 5. 11.0
_ _ _ _ _ 6. 4.1 (tomato)
_ __ _ _ 7. -0.32
pOH = -(log [OHl)
Just as pH expresses the concentration of the hydrogen ion, pOH
expresses the concentration of the hydroxide ion in an aqueous
solution. At room temperature, the sum of pH and pOH equals 14.
pH+pOH= 14
[H30j [OHl
= 1 x 1o- 14
8. Determine the missing information.
[H30+]
pH
[OH1
pOH
Acid, base or
neutral?
7
3.5
X
10" 12M
2.6
9. Acid-base (pH) indicators are compounds whose color varies with pH. At each given pH, state the
indicator's color.
[H 30+)
8.7
X
pH
10"11 M
4.52
10"7 M
Litmus
Phenolphthalein
Acid, base or
neutral?
-:~
Nrune ____________________________________
Class _____
:::__ -= -
Date - --------
Acid-Base Theories
1.
Summarize the three main acid-base theories in the table below.
ACID
BASE
Arrhenius
Br0nsted-Lowry
Lewis
Use the following chemical equations to answer question 2.
NH3 + H20 ~NIL.++ OH-
HCl + H20-+ H30+ + Cl-
and NH3 would be classified as
2. According to Arrhenius, HCl would be classified as a(n)
a(n)
. Explain why.
For problems 3- 5, label the acid (A), base (B), conjugate acid (CA), and conjugate base (CB) in each of
the following reactions. Show the transfer of the proton (H) by drawing an arrow.
For problems 6- 9, give the conjugate base for each Bransted.-Lowry acid.
6. HI
8. HzC03
7. NH/
9. HN03
For problems 10- 13, give the conjugate acid for each Bransted-Lowry base.
10. CN-
12.
cH3coo-
13. NH3
-
--
--
-~- -~;_,;,_ :: - ; ~C'. :;,~--·
'-·
-
..
Use the following diagram to answer question 14.
H
I /""'., I ..
...,B-F:
I ..
I
H-N:'
H
..
H :p:
!F!
:p:
----7
I I
I I ..
H-N-B-F:
..
H :F:
14. The Lewis acid in the above equation is - -- - -- - · The Lewis base is _ _ _ _ __
Explain why.