pH Calculations
pH 1
What is the pH of 2.2 x 10-2 M
hydrochloric acid solution?
Dissociation, Neutralization Reactions
D, N 1
Show the dissociation of
HBr  ____ + ____
Titrations
T1
In a titration, 20 mL of 2.0 M HCl reacted
with 25 mL of NaOH. What was the
concentration of the sodium hydroxide?
Acids & Bases
A, B 1
Acids dissociate into ____ ions, bases
dissociate into ____ ions.
pH 2
A solution of the strong acid HClO4 has a
hydrogen ion concentration of 1 x 10-3M.
What is the pH of this solution?
D, N 2
Show the dissociation of
KOH  ____ + ____
T2
In a titration, 20 mL of 0.2 M HCl reacted
with 50 mL of NaOH. What was the
concentration of the sodium hydroxide?
A, B 2
Compare and contrast 3 properties of
acids and 3 properties of bases.
pH 3
Benzoic acid has an [H+] as 6.3 x 10-5.
What is the pH of this solution?
D, N 3
Describe the difference between strong
and weak acids in terms of dissociation.
T3
In a titration, 20 mLof 0.15 M HCl reacted
with 25 mL of NaOH. What was the
concentration of the sodium hydroxide?
A, B 3
List household examples of 2 acids and
list examples of 2 bases.
pH 4
Citric acid has an [H+] of 8.13 x 10-4, what
is the pH of citric acid?
D, N 4
What is a neutralization reaction?
T4
In a titration, 20 mL of 1.14 M HCl reacted
with 25 mL of NaOH. What was the
concentration of the sodium hydroxide?
A, B 4
What is the purpose of an indicator?
Give an example of an indicator and
describe how you know if the solution is
acidic or basic.
pH 5
The hydrogen ion concentration dilute
vinegar is 1.3 x 10-6. What is the pH of this
solution?
D, N 5
Write the neutralization equation:
T5
10.0 mL of a solution of potassium
hydroxide was titrated with 13.5mL of a
0.10 M solution of hydrochloric acid.
Calculate the concentration of KOH.
A, B 5
What is the purpose of a titration?
pH 6
A sample of rain has an [H+] of 6.31 x 10-6.
What is the pH of the sample?
D, N 6
Write the neutralization equation:
T6
Calculate the concentration of an acetic
acid solution if 34.57 mL of this solution is
needed to neutralize 25.19 mL of a
0.1025 M sodium hydroxide.
A, B 6
Describe the procedure for a titration.
T7
25.00mL of 0.100M NaOH is needed to
titrate 25.00mL of a solution of
hydrochloric acid. Calculate the
concentration of the acid.
A, B 7
Name 2 acids and 2 bases.
T8
23.15mL of 0.125M NaOH is needed to
titrate 25.00mLof a solution of
hydrochloric acid. Calculate the
concentration of the acid.
A, B 8
What does pH measure?
HNO3 + NaOH  ___________________
HC2H3O2 + LiOH  __________________
pH 7
What is the pH of sodium hydroxide
(strong base) if [H+] = 2.0 x 10-12?
D, N 7
Write the neutralization equation:
H3PO4 + KOH  ___________________
pH 8
What is the concentration of the strong
base, potassium hydroxide, if the
hydroxide ion concentration of the
solution is 6.3 x 10-11?
D, N 8
Write the neutralization equation:
HClO3 + Ca(OH)2  _________________