Unit 17 Acids and Bases Study Guide
Name __________________________ Date _______
1) What is the Arrhenius definition of an acid? Give an example.
2) What is the Arrhenius definition of a base? Give an example.
3) What is the Bronsted-Lowry definition of an acid?
4) What is the Bronsted-Lowry definition of a base?
5) What are the properties (characteristics) of an acid?
6) What are the properties (characteristics) of a base?
7) Bases are compounds that react with acids to form ________________ and a(n) _____________.
8) Is the following sentence true or false? Some of the acids and bases included in the Arrhenius theory
are not acids and bases according to the Brønsted-Lowry theory.
9) What is a conjugate acid-base pair?
10) What does a water molecule that loses a hydrogen ion become?
11) What does a water molecule that gains a hydrogen ion become?
12) Is the following sentence true or false? Any aqueous solution in which [H+] and [OHí]
are equal is described as a neutral solution.
13) A(n)
solution is one in which [H+] is greater than [OHí]. A(n) ___________ solution
is one in which [H+] is less than [OHí].
14) Match the type of solution with its hydrogen-ion concentrations.
______________ acidic
a. less than 1.0 × 10íM
_______________ neutral
b. greater than 1.0 × 10íM
_______________ basic
c. 1.0 × 10íM
15) What is the formula for pH?
16) What is the formula for pOH?
17) How do you determine the pH from the pOH?
18) If you were given the pH or the pOH and wanted to determine the concentration of either H+ or OHions, what would be the formula?
19) What are the ranges for the pH scale?
20) What are the ranges for the pOH scale?
21) Is the following sentence true or false? Most pH values are whole numbers.
22) Why is an indicator a valuable tool for measuring pH?
23) Why do you need many different indicators to span the entire pH spectrum?
24) List at least three characteristics that limit the usefulness of indicators.
25) What are three strong acids?
26) What are three strong bases?
27) Is the following sentence true or false? Acids react with compounds containing
hydroxide ions to form water and a salt.
28) Salts are compounds consisting of a(n) ________________ from an acid and a(n) ____________
from a base.
29) Complete the flow chart below showing the steps of a neutralization reaction.
A measured volume of an acid solution of
added to a flask.
Several drops of the
gently swirled.
Measured volumes of a base of
the acid until the indicator changes
concentration is
are added to the solution while the flask is
concentration are mixed into
.
30) The process of adding a known amount of solution of known concentration to determine the
concentration of another solution is called _________________
Practice Problems
Acid
Base
Conjugate
Acid
Conjugate
Base
Equation
1)
HNO3
H2O
H3O+
NO2-
HNO2 + H22ĺ122- + H3O+
2)
H2O
F-
HF
OHNH3 +&1ĺ1+4+ + CN-
3)
H2O
4)
5)
HSO4-
ClO3-
PO43S2- + H22ĺ2+- + HS-
6)
7)
A solution has a hydrogen ion concentration of 1 × 10–6M. What is its pH?
8)
A solution has a pOH of 5.68. What is the concentration of hydrogen ions?
9)
What is the pH of a solution if the [H+] = 7.2 × 10–9M?
10) What is the pOH of a solution if the [OH–] = 3.5 × 10–2M?
11) What is the pOH of a solution that has a pH of 3.4?
12) Classify each solution as acidic, basic, or neutral.
a. [H+] = 2.5 × 10–9M
d. [H+] = 1 × 10–7M
b. pOH = 12.0
e. pH = 0.8
c. [OH–] = 9.8 × 10–11M
13) Calculate the pH of each solution.
a. [H+] = 1 × 10–5M
b. [H+] = 4.4 × 10–11M
c. [OH–] = 2.2 × 10–7M
d. pOH = 1.4
14) A solution has a pOH of 12.4. What is the pH of this solution?
15) What is the pH of a solution with [H–] = 1 × 10–3M?
16) What color does litmus paper turn for acids? For bases?
17) Where can you find strong acids on the pH scale?
18) Where can you find strong bases on the pH scale?
19) Where are the weak acids and weak bases?
20) What is the titrant?
21) What is an analyte?
22) Which solution below has the highest concentration of hydroxide ions and why?
c. pH = 12.6
a. pH = 9.82
b. pH = 3.21
d. pH = 7.93
23) If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration
of the HCl?
24) Titration of 25.00 mL of 0.100 M NH3 with 0.100 M HCl (weak base, strong acid):
a. Circle the equivalence point and define it.
b. Why is pH < 7 at the equivalence point for this graph?
25) Draw a strong acid (HCl) completely dissociated in water. Draw a weak acid partially dissociated in
water.
26) It takes 83 mL of a 0.45 M NaOH solution to neutralize 235 mL of an HCl solution. What is the
concentration of the HCl solution?
27) It takes 38 mL of 0.75 M NaOH solution to completely neutralize 155 mL of a sulfuric acid solution
(H2SO4). What is the concentration of the H2SO4 solution?
28) What is the pH of a 3.0 M HF (assume 10% dissociation)?