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1
CHEMISTRY 103 – WORKSHEET #3 – Module 3
Chemical Reactions
Do the topics appropriate for your course
Prepared by Dr. Tony Jacob
https://clc.chem.wisc.edu
(Resource page)
ACIDS:
Produce H
+
in solution; for Chem 103 acids
begin with H
(except H
2
O) or
contain: –COOH
STRONG ACIDS
(
best to
memorize
): HCl, HBr, HI, HNO
3
, HClO
4
, H
2
SO
4
(note: H
2
SO
4
(aq)
®
H
+
(aq) + HSO
4
-
(aq))
WEAK ACIDS
(
best to
memorize
): CH
3
COO
H
(acetic acid); H
3
PO
4
(phosphoric acid);
H
2
CO
3
(carbonic acid)
BASES:
Produce OH
-
in solution (e.g., NaOH(aq)
®
Na
+
(aq) + OH
-
(aq))
STRONG BASES
: LiOH, NaOH, KOH; Ca(OH)
2
, Sr(OH)
2
, Ba(OH)
2
WEAK BASES
: NH
3
ELECTROLYTES:
Chemicals that generate ions
Strong electrolytes
= large number of ions:
1. strong acids, 2. strong bases, 3. soluble ionic compounds
Weak electrolytes
= small number of ions:
1. weak acids, 2. weak bases
Nonelectrolytes
= no ions:
1. molecular compounds, 2. insoluble ionic compounds
CONDUCTIVITY TEST:
a light bulb dipped into a solution is used to test conductivity;
bright light:
strong electrolyte/many ions
(strong acids, strong bases, soluble ionic compounds)
dim light:
weak electrolyte/small ions. (weak acids, weak bases)
no light:
nonelectrolyte/no ions. (insoluble ionic compounds, molecular compounds)
Solubility Rules
Soluble
Exceptions
Insoluble
Exceptions
Li
+
, Na
+
, K
+
, Rb
+
, Cs
+
, NH
4
+
OH
-
, CO
3
2-
, PO
4
3-
, S
2-
Li
+
, Na
+
, K
+
, Rb
+
, Cs
+
, NH
4
+
NO
3
-
, ClO
3
-
, ClO
4
-
, CH
3
COO
-
CrO
4
2-
Li
+
, Na
+
, K
+
, Rb
+
, Cs
+
, NH
4
+
, Mg
2+
Cl
-
, Br
-
, I
-
Ag
+
, Pb
2+
, Hg
2
2+
SO
4
2-
Ca
2+
, Sr
2+
, Ba
2+
, Pb
2+
WRITING REACTIONS (steps)
I.
Molecular Reaction:
All compounds are written in a molecular form; no ions.
1.
Names
®
formulas (if needed)
2.
Assign charges and balance reactant formulas
3.
For products: Switch partners; use
only 1 of each ion initially
4.
Assign charges to product formulas and balance product formulas
5.
Balance reaction
II.
Complete Ionic Reaction:
Break all appropriate chemicals into ions
Break up
1. strong acids
(memorized)
2. strong bases
(memorized)
3. soluble ionic compounds
(solubility rules)
Don't break up
1. weak acids
(acids that are not strong acids)
2. weak bases
(bases that are not strong bases)
3. insoluble ionic compounds
(solubility rules)
4. molecular compounds
(2 or more nonmetals)
Unusual ones: H
2
CO
3
(aq)
®
H
2
O(l) + CO
2
(g); H
2
SO
3
(aq)
®
H
2
O(l) + SO
2
(g); H
2
SO
4
(aq)
®
H
+
(aq) + HSO
4
-
(aq)
III.
Net Ionic Reaction
: Cross out common ions (spectator ions); if everything cancels out
®
no reaction
H
+
A
-
H
+
A
-
H
+
A
-
H
+
A
-
A
-
H
+
H
A
H
A
H
A
2
TYPES OF REACTIONS
Precipitation (ppt)
: MA(aq) + NB(aq)
®
MB(aq) + NA
(s)
Acid/Base
: acid(aq) + base(aq)
®
salt(aq) + H
2
O(l)
Gas forming
: [HCO
3
-
(aq) or CO
3
2-
(aq)] + H
+
(acid)(aq)
®
H
2
CO
3
(aq)
®
H
2
O(l) + CO
2
(g)
(see below)
Combustion
:
C
x
H
y
(O
z
) + O
2
(g)
®
CO
2
(g) + H
2
O(g)
(can be C
x
H
y
(O
z
) or C
x
H
y
)
Redox
: change in oxidation number
TYPES OF REACTIONS
(examples of molecular, complete ionic, and net ionic reactions for each type of reaction)
1.
Precipitation
2 aqueous solutions switch partners:
produce a solid and a salt (salt = soluble ionic compound)
Example 1:
Barium nitrate and potassium sulfate are mixed.
Write the molecular, complete ionic and net ionic reactions.
Answer 1:
Ba(NO
3
)
2
(aq) + K
2
SO
4
(aq)
®
BaSO
4
(s) + 2KNO
3
(aq)
(
molecular reaction
)
Ba
2+
(aq) + 2NO
3
-
(aq) + 2K
+
(aq) + SO
4
2-
(aq)
®
BaSO
4
(s) + 2K
+
(aq) + 2NO
3
-
(aq)
(
complete ionic reaction
)
Ba
2+
(aq) + SO
4
2-
(aq)
®
BaSO
4
(s)
(
net ionic reaction
)
2.
Acid/Base (neutralization)
Acid + Base
®
H
2
O + salt;
acid and base
switch partners: usually produce H
2
O and a salt
Example 2:
Nitric acid and sodium hydroxide are mixed (strong acid (SA) + strong base (SB)).
Write the molecular, complete ionic and
net ionic reactions.
Answer 2:
SA + SB:
HNO
3
(aq) + NaOH(aq)
®
H
2
O(l) + NaNO
3
(aq)
(
molecular reaction
)
H
+
(aq) + NO
3
-
(aq) + Na
+
(aq) + OH
-
(aq)
®
H
2
O(l) + Na
+
(aq) + NO
3
-
(aq)
(
complete ionic reaction
)
H
+
(aq) + OH
-
(aq)
®
H
2
O(l)
(net ionic reaction)
Example 3:
Acetic acid and lithium hydroxide are mixed (weak acid (WA) + strong base (SB)).
Write the molecular, complete ionic
and net ionic reactions.
Answer 3:
WA + SB:
CH
3
COOH(aq) + LiOH(aq)
®
H
2
O(l) + LiCH
3
COO(aq)
(
molecular reaction
)
CH
3
COOH(aq) + Li
+
(aq) + OH
-
(aq)
®
H
2
O(l) + CH
3
COO
-
(aq) + Li
+
(aq)
(
complete ionic reaction
)
CH
3
COOH(aq) + OH
-
(aq)
®
H
2
O(l) + CH
3
COO
-
(aq)
(
net ionic reaction
; note difference from SA+SB (example 2) vs WA+SB)
3.
Gas-Forming
•
Carbon dioxide gas
, CO
2
: acid (H
+
) + CO
3
2-
(aq)
®
H
2
CO
3
(aq)
®
H
2
O(l) + CO
2
(g)
•
Sulfur dioxide gas
, SO
2
: acid (H
+
) + SO
3
2-
(aq)
®
H
2
SO
3
(aq)
®
H
2
O(l) + SO
2
(g)
•
Dihydrogen sulfide gas
, H
2
S: acid (H
+
) + S
2-
(aq)
®
H
2
S(g)
•
Hydrogen gas
, H
2
: metal(s) + H
2
O(l) or acid (H
+
)
®
M
+
(aq) + OH
-
(aq) + H
2
(g) (this is also a redox reaction)
Example 4:
Hydrochloric acid and sodium carbonate are mixed.
Write the molecular, complete ionic and net ionic reactions.
Answer 4:
2HCl(aq) + Na
2
CO
3
(aq)
®
H
2
CO
3
(aq) + 2NaCl(aq)
H
2
CO
3
(aq) breaks up: H
2
CO
3
(aq)
®
H
2
O(l) + CO
2
(g)
to yield:
2HCl(aq) + Na
2
CO
3
(aq)
®
H
2
O(l) + CO
2
(g) + 2NaCl(aq)
(
molecular reaction
; CO
2
(g) is the gas in this gas-forming reaction)
2H
+
(aq) + 2Cl
-
(aq) + 2Na
+
(aq) + CO
3
2-
(aq)
®
H
2
O(l) + CO
2
(g) + 2Na
+
(aq) + 2Cl
-
(aq)
(
complete ionic reaction
)
2H
+
(aq) + CO
3
2-
(aq)
®
H
2
O(l) + CO
2
(g)
(
net ionic reaction
)
4.
Combustion
C
x
H
y
(O
z
) +
O
2
(g)
®
CO
2
(g) + H
2
O(g)
{the bold part of this reaction is unchanged in other combustion reactions}
Example 5:
Octane, C
8
H
18
, is burned.
Write the molecular, complete ionic and net ionic reactions.
Answer 5:
2C
8
H
18
(g) + 25O
2
(g)
®
16CO
2
(g) + 18H
2
O(g)
(
molecular reaction
; when balancing: first balance C, then H, then O)
2C
8
H
18
(g) + 25O
2
(g)
®
16CO
2
(g) + 18H
2
O(g)
(
complete ionic reaction
)
2C
8
H
18
(g) + 25O
2
(g)
®
16CO
2
(g) + 18H
2
O(g)
(
net ionic reaction
)
5.
Redox (see the next page)
oxidation numbers change as chemicals go from reactants to products
3
REDOX
1.
Assign Oxidation Numbers
1.
Elements = 0
2.
In a compound:
a. Group 1A (Li, Na,...)
+1 (always)
b. Group 2A (Be, Mg,...)
+2 (always)
c. F
-1 (always)
d. H
+1 (usually; can also be –1 with MH
x
; (e.g., NaH))
e. O
-2 (usually; can also be: –1 with O
2
2-
(e.g., H
2
O
2
);
–
1
/
2
with O
2
-
(e.g., KO
2
); +1 with F (e.g., F
2
O
2
))
3.
Sum Rule: Sum of all the oxidation numbers = total charge on the compound
2.
Identify:
chemical oxidized, reduced, oxidizing agent, reducing agent; must be
reactants
(no products)
LEO
the lion goes GER
(LEO = lose e
-
oxidized; GER = gain e
-
reduction)
If oxidation numbers going from reactants
®
products get
more positive
Þ
reactant is oxidized
If oxidation numbers get
more negative
Þ
reactant is reduced
Hint: What is oxidized is also the reducing agent; what is reduced is also the oxidizing agent.
Example 6:
a. In the reaction shown, what is oxidized, reduced, oxidizing agent, and reducing agent?
b. How many electrons were transferred in the reaction?
Cu(s) + 2HNO
3
(aq)
®
CuO(s) + 2NO
2
(g) + H
2
O(l)
Answer 6:
a. Cu(s) = oxidized, HNO
3
(aq) = reduced, oxidizing agent = HNO
3
(aq), reducing agent = Cu(s)
{Cu: 0
®
+2: becoming more positive
®
oxidized; N in HNO
3
: 5
®
4: becoming more negative
®
reduced;
HNO
3
is reduced
®
oxidizing agent; Cu is oxidized
®
reducing agent}
b. 2 electrons transferred
{Cu: 0
®
2: 2e
-
;
or
N: 5
®
4: 1e
-
;
}
3.
Is it a Redox Rxn?
Redox reaction occurs when oxidation numbers change in a reaction.
Hints:
•
If reaction has an
element
on one side and that element
is in a compound
on the other side
®
nearly
always a
redox reaction
•
If reaction is a
combustion
reaction
®
redox reaction
•
If reaction is an
acid/base
,
precipitation
, or
gas-forming
reaction (except for metal + (H
+
or H
2
O))
®
not a redox reaction
reduction
oxidation
-
+
0
change in
oxidation numbers
2e
−
Cu atom
1Cu atom
(
)
=
2e
−
lost
1e
−
N atom
2 N atom
(
)
=
2e
−
gained
CuO(s)
+
2NO
2
(g)
+
H
2
O(l)
Cu(s)
+
2HNO
3
(aq)
0
1 5 -2
2 -2
4 -2
1 -2
reduction
oxidation
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4
4.
Metal Activity Series
– a list of how easily a metal is oxidized; a metal higher on the list
will react
with
an ion lower on the list (
down and to the right
); reactions that are
up and to the right
will
not occur
Reactions Occur:
Mn(s) + FeBr
2
(aq)
®
MnBr
2
(aq) + Fe(s)
Þ
reaction occurs
since down and to the left on the activity series
2Cr(s) + 6HBr(aq)
®
2CrBr
3
(aq) + 3H
2
(g)
Þ
reaction occurs
since down and to the left on the activity series
Reactions Don’t Occur: Cu(s) + Cr
3+
(aq)
Þ
no reaction occurs
since up and to the right on the activity series
Fe(s) + Mn
2+
(aq)
Þ
no reaction occurs
since up and to the right on the activity series
Reaction Occurs
When metal is
above
the cation
No Reaction Occurs
When metal is
below
the cation
1. Which of the following is a
weak acid
and
strong base
reaction?
a. HF(aq) + NH
3
(aq)
®
NH
4
+
(aq) + F
-
(aq)
b. Ba(OH)
2
(aq) + 2HCl(aq)
®
Ba
2+
(aq) + 2Cl
-
(aq) + 2H
2
O(l)
c. H
3
PO
4
(aq) + 3LiOH(aq)
®
3Li
+
(aq) + PO
4
3-
(aq) + 3H
2
O(l)
d. CH
3
COOH(aq) + NH
3
(aq)
®
CH
3
COO
-
(aq) + NH
4
+
(aq)
e. None of the above reactions match the above statement.
2. Which reaction is the
balanced molecular reaction
for iron(II) nitrate reacting with sodium sulfide to
form a precipitate?
a. NO
3
-
(aq) + Na
+
(aq)
®
NaNO
3
(aq)
b. Fe
2
(NO
3
)(aq) + NaS(aq)
®
Fe
2
S(s) + NaNO
3
(aq)
c. Fe(NO
3
)
2
(aq) + Na
2
S(aq)
®
FeS(s) + 2NaNO
3
(aq)
d. 2Fe(NO
3
)
2
(aq) + Na
2
S(aq)
®
2FeNa(s) + S(NO
3
)
4
(aq)
e. Fe
2+
(aq) + 2NO
3
-
(aq) + 2Na
+
(aq) + S
2-
(aq)
®
FeS(s) + 2Na
+
(aq) + 2NO
3
-
(aq)
3. What is the
sum of the coefficients
for the
balanced combustion reaction
for propanol, C
3
H
8
O(l)?
a. 6
b. 11
c. 13
d. 25
e. None of these are correct.
Mn(s)
Mn
2+
(aq) + 2e
-
Cr(s)
Cr
3+
(aq) + 3e
-
Fe(s)
Fe
2+
(aq) + 2e
-
Cu(s)
Cu
2+
(aq) + 2e
-
H
2
(g)
2H
+
(aq) + 2e
-
Al(s)
Al
3+
(aq) + 3e
-
Zn(s)
Zn
2+
(aq) + 2e
-
More Easily Oxidized
Mn(s)
Mn
2+
(aq) + 2e
-
Cr(s)
Cr
3+
(aq) + 3e
-
Fe(s)
Fe
2+
(aq) + 2e
-
Cu(s)
Cu
2+
(aq) + 2e
-
H
2
(g)
2H
+
(aq) + 2e
-
Al(s)
Al
3+
(aq) + 3e
-
Zn(s)
Zn
2+
(aq) + 2e
-
5
4. What is the
oxidation number
of
sulfur
in S
2
O
3
2-
?
a. 6
b. -3
c. 4
d. 2
e. 3
5. Using the chemical reaction shown select which statements are
CORRECT
.
8S
2-
(aq) +
16NO
3
-
(aq)
+ 32H
+
(aq)
®
16NO
2
(g)
+
S
8
(s)
+
16H
2
O(l)
i. S
2-
is oxidized
ii. N in NO
3
-
is oxidized
iii. NO
3
-
is the oxidizing agent
a. i
b. i, ii
c. ii, iii
d. i, iii
e. i, ii, iii
6. Which reaction is the
balanced net ionic reaction
for the reaction of acetic acid and sodium hydroxide?
a. H
+
(aq) + OH
-
(aq)
®
H
2
O(l)
b. CH
3
COOH(aq) + NaOH(aq)
®
CH
3
COONa(aq) + H
2
O(l)
c. CH
3
COOH(aq) + OH
-
(aq)
®
CH
2
COOH(aq) + H
2
O(l)
d. CH
3
COOH(aq) + OH
-
(aq)
®
CH
3
COO
-
(aq) + H
2
O(l)
e. H
+
(aq) + NaOH(aq)
®
Na
+
(aq) + H
2
O(l)
7. The following compounds were used in a conductivity test.
Which will cause the
light
bulb to shine
brightly
when dissolved in water?
i. lead(II) chloride
ii. potassium fluoride
iii. acetic acid
a. i
b. ii
c. iii
d. i, ii
e. i, iii
f. ii, iii
6
8. When ammonia gas reacted with oxygen gas over a catalyst, nitrogen gas and water were formed.
What chemical is the
reducing agent
?
(Hint 1: Write the chemical reaction.
Hint 2: No need to balance;
stoichiometric coefficients not used when assigning oxidation numbers.)
a. ammonia gas
b. oxygen gas
c. nitrogen gas
d. water
e. the catalyst
9. Use the table below with the given chemical reaction observations to
determine the unknown
chemicals A and B
.
There are three possibilities for the unknown chemical shown in the last row:
BaCO
3
, AgNO
3
, and Fe(NO
3
)
2
.
Chemical mixed
with the Unknown
Unknown A
Unknown B
HCl
Bubbles
Precipitate
KOH
No observed change
Precipitate
H
2
SO
4
Precipitate; bubbles
No observed change
Unknowns:
BaCO
3
AgNO
3
Fe(NO
3
)
2
BaCO
3
AgNO
3
Fe(NO
3
)
2
a. Unknown A = BaCO
3
, Unknown B = AgNO
3
b. Unknown A = BaCO
3
, Unknown B = Fe(NO
3
)
2
c. Unknown A = AgNO
3
, Unknown B = Fe(NO
3
)
2
d. Unknown A = AgNO
3
, Unknown B = BaCO
3
e. Unknown A = Fe(NO
3
)
2
, Unknown B = BaCO
3
f. Unknown A = Fe(NO
3
)
2
, Unknown B = AgNO
3
10. Which of the following reactions
are redox reactions
?
i. C
2
H
4
(g) + 3O
2
(g)
®
2CO
2
(g) + 2H
2
O(g)
ii. Al(s) + Fe(NO
3
)
3
(aq)
®
Al(NO
3
)
3
(aq) + Fe(l)
iii. N
2
(g) + 3O
2
(g)
®
2NO
3
(g)
a. i
b. ii
c. iii
d. i, ii
e. i, iii
f. ii, iii
g. i, ii, iii
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7
CHEMISTRY 103 – WORKSHEET #3 - ANSWERS
Chemical Reactions
Do the topics appropriate for your lecture
Prepared by Dr. Tony Jacob
https://clc.chem.wisc.edu
(Resource page)
ANSWERS
1. c
{“a”: weak acid + weak base; “b”: strong acid + strong base; “c”: weak acid + strong base; “d”: weak acid + weak base}
2. c
{converting names to formulas: iron(II) = Fe
2+
; nitrate = NO
3
-
; iron(II) nitrate = Fe(NO
3
)
2
;
sodium = Na
+
; sulfide = S
2-
; sodium sulfide = Na
2
S; switch partners to yield (Fe
2+
)(S
2-
) and balance = FeS, and
(Na
+
)(NO
3
-
) and balance = NaNO
3
; these are the two products; for molecular reactions the chemicals are kept in their
molecular form and are not broken into
ions
; since reactions “a” and “e” have ions they are not correct;
reaction “b” has the wrong individual formulas in both reactants and products: for instance, NaS rather than Na
2
S;
reaction “d” the product formed contain 2 cations (Fe
2+
)(Na
+
) and 2 anions (S
2-
)(NO
3
-
) which is incorrect;
only reaction “c” has the correct chemical formulas and is not broken into ions}
3. d
{combustion reactions: C
x
H
y
O
z
+ O
2
(g)
®
CO
2
(g) + H
2
O(g); C
3
H
8
O(l) + O
2
(g)
®
CO
2
(g) + H
2
O(g); when
balancing combustion reactions balance in the order: C, H, then O:
Balance C: C
3
H
8
O(l) + O
2
(g)
®
3CO
2
(g) + H
2
O(g);
Balance H: C
3
H
8
O(l) + O
2
(g)
®
3CO
2
(g) + 4H
2
O(g);
Balance O: C
3
H
8
O(l) +
9
/
2
O
2
(g)
®
3CO
2
(g) + 4H
2
O(g); get rid of fraction by multiplying entire reaction by 2:
2C
3
H
8
O(l) + 9O
2
(g)
®
6CO
2
(g) + 8H
2
O(g); coefficients: 2 + 9 + 6 + 8 = 25}
4. d
{sum of the oxidation numbers = charge: 2S + 3O = -2; 2(x) + 3(-2) = -2; 2x - 6 = -2; 2x = 4; x = 2}
5. d
{S
2-
: S = -2; S
8
: S = 0; S: -2
®
0
®
S
2-
oxidized = reducing agent; therefore choice “i” is
true
;
NO
3
-
: N = +5; NO
2
: N = +4; N: +5
®
+4
®
N is reduced = oxidizing agent; therefore choice “ii” is
false
and
choice “iii” is
true
; option “d” has “i” and “iii”}
6. d
{CH
3
COOH is a weak acid so it does not break up and therefore answers “a” and “e” are
incorrect
;
the acidic H is the H bolded/underlined: CH
3
COO
H
therefore answer “c” is
incorrect
because the wrong H came off as
shown in the product formula; answer “b” is a correctly written reaction, but it represents the molecular reaction rather
than the net ionic reaction; the correct answer is “d” with the
correct
H being removed from CH
3
COO
H
, NaOH being
broken up (strong base) and the Na
+
being canceled out as it is a spectator ion}
7. b
{“i”: lead(II) chloride = PbCl
2
is an
insoluble ionic compound
: non-electrolyte therefore
no light
;
“ii”: potassium fluoride = KF is a
soluble ionic compound
: strong electrolyte therefore
bright light
;
“iii”: acetic acid = CH
3
COOH is a
weak acid
: weak electrolyte therefore
dim light
}
8
8. a
{write the reaction: 4NH
3
(g) + 3O
2
(g)
®
2N
2
(g) + 6H
2
O(l); Note: the reaction
does not
need to be balanced
; only
the correct formulas for each chemical is needed since the stoichiometric coefficients are not used when assigning
oxidation numbers; assign oxidation numbers:
; what is oxidized: NH
3
: N: goes from -3 to 0; reduced: O
2
: O: goes from 0 to -2;
oxidizing agent: O
2
(same as what is reduced); reducing agent: NH
3
(same as what is oxidized); all must be
reactants
}
9. a
{
Unknown A must be BaCO
3
as a carbonate, CO
3
2-
, when combined with an acid like HCl will form H
2
CO
3
which
then breaks into CO
2
(g) and H
2
O(l).
Neither AgNO
3
nor Fe(NO
3
)
2
will generate any bubbles with HCl.
Unknown B
must be AgNO
3
since AgNO
3
mixed with HCl will form AgCl(s) which is insoluble and forms a precipitate.
To contrast,
BaCO
3
mixed with HCl will form BaCl
2
which is soluble and does not form a precipitate.
Likewise, Fe(NO
3
)
2
mixed
with HCl will form FeCl
2
which is soluble and does not form a precipitate.}
10. g
{Rxn i: combustion reaction which is a redox reaction; also oxidation number of O starts at 0 in O
2
and goes to -2 in
both CO
2
(g) and H
2
O; change in oxidation number
®
redox; can also focus on C: -2 in C
2
H
4
to +4 in CO
2
®
redox!
Rxn ii: for Al(s): Al = 0; for Al in Al(NO
3
)
3
(aq): Al = +3 since the charge on NO
3
-
is -1; so Al goes from 0 to +3
®
redox!
can also focus on Fe: goes from +3 in Fe(NO
3
)
3
to 0 in Fe(l)
®
redox!
Rxn iii: N in N
2
(g): N = 0 while in NO
3
-
, N has an oxidation number of +6; change in oxidation number
®
redox; can
also focus on O: goes from 0 in O
2
®
-2 in NO
3
-
®
redox}
+
+
4NH
3
(g)
3O
2
(g)
2N
2
(g)
6H
2
O(l)
+1
-3
0
0
+1 -2
oxidized
reduced
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try 02 Fa 20 CHEM1310 02_Fa_20
Module 11
11. Reactions of Acids and Bases
...
Identify types of reactions involving acids and bases
Question
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4.
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4.Suppose you run a titration of an acid yourself. You do it three times be-
tween an acid and sodium hydroxide solution. Here is some data:
Average volume of sodium hydroxide solution delivered: 9.10 mL
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Average mass of acid solution: 9.555 g
The average volume of sodium hydroxide solution is the average of three titra-
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The same goes for the average mass of the acid. You ran the experiment three
times and the average mass of the acid solution is given for those three titra-
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a)
b)
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