WorksheetsUnit 11 Pretest Acid and Base
Total questions: 28
Worksheet time: 14mins
Which of the following is the correct formula for carbonic acid?
HCO3
HCO
HCO₂
H2CO3
Which of the following is the correct formula for acetic acid?
HC₂H₃O₂
HC₃H₃O₃
H₂C₃H₂O₃
H₃As
Which best represents the subscripts on the correct formula for phosphoric acid, H1234P1234O1234?
2 1 4
3 1 4
313
Which of the following is the correct formula for the base calcium hydroxide?
Ca(OH)₂
Ca₂OH
Ca(OH)₃
CaOH
Which of the following is paired CORRECTLY?
hydrochloric acid, HClO₄
Nitric acid, H₂SO₄
Sulfuric acid, H₂SO₄
Perchloric acid, HNO₃
Which of the following is correct about the naming of acids?
The prefix “hydro-” is used when the acid contains oxygen.
The suffix “-ous” is used when the anion ends in “-ate”.
The suffix “-ic” is used when the anion ends in “-ate”.
All acids have the prefix “hydro-”.
A titration of 30.0 mL of H2SO4 is completed after adding 15.0 mL of 0.200 M KOH. What is the concentration of the sulfuric acid?
0.10 M
0.20 M
0.30 M
0.40 M
What is the molarity of 65 mL of lithium hydroxide, LiOH, if 95 mL of 0.50 M hydrosulfuric acid, H₂S, neutralizes it?
1.46 M
0.731 M
0.684 M
0.342 M
Which of the following describes a weak electrolyte?
A solution where the solute completely dissociates.
A solution where the solute does not dissociate at all.
A solution where the solute partially dissociates.
A solute that dissolves but does not dissociate.
Which of the following is a Brønsted–Lowry acid?
OH⁻
H₂O
NH₃
HCl
Which of the following substances will have a pH greater than 7.0?
H₂SO₄
NaOH
CH₃COOH
HCl
A solution of HCl has a concentration of 1.0 x 10^-4. What is the pH of the solution?
1.0 x 10^-4
1.0 x 10^-10
4.0
10.0
What volume of 0.15 M potassium hydroxide is required to completely neutralize 150.0 mL of 0.1 M sulfuric acid?
50 mL
100 mL
200 mL
150 mL
Which of the following aqueous solutions cannot exist at 25 °C?
pH= 7.0, pOH= 7.0
pH= 11.0, pOH= 3.0
pH= -1.0, pOH= 15.0
pH= 1.0, pOH= 6.0
Which of the following is true about a neutral solution?
There are no H⁺ or OH⁻ ions in a neutral solution.
The concentration of H⁺ and OH⁻ are equal.
The pH of a neutral solution is 0.
The [ H⁺ ] is larger than the [ OH⁻ ].
An aqueous solution of an ionic compound turns blue litmus red, conducts electricity, and reacts with a base to form a salt and water. Which compound would this most likely be?
NaOH
H₂SO₄
CaCl₂
NH₄NO₃
According to the Arrhenius Theory, a substance that is classified as a base will always yield (a) .
In an aqueous solution that is acidic, which relationship between ion concentrations always exists?
[ H⁺ ] is greater than [ OH⁻ ]
[ H⁺ ] equals zero
[ H⁺ ] equals [ OH⁻ ]
[ H⁺ ] is less than [ OH⁻ ]
What is the pH of a solution with a hydroxide ion concentration of 1 x 10⁻⁶ M?
8
6
12
4
What is the pH of a 0.001 M solution of NaOH?
3
11
7
14
Use the equation below to answer the question. HNO₂ (aq) + H₂O (l) → H₃O⁺¹ (aq) + NO₂⁻¹ (aq) Which of the following represents the conjugate base?
HNO₂
H₂O
H₃O⁺¹
NO₂⁻¹
Which of the following indicates the most acidic solution?
[H⁺] = 1 x 10⁻⁵
pOH = 9.8
pH = 2.3
[OH⁻] = 1 x 10⁻⁶ M
In the reaction below, the NH₃ is acting as __________________________. NH₃ + H₂O → NH₄⁺ + OH⁻
a proton acceptor only
a proton donor only
both a proton acceptor and donor
neither a proton donor nor an acceptor
Which of the following is a property of an acid?
Acids increase the amount of H⁺ ions in a solution.
Acids decrease the conductivity of solutions.
Acids have a pH greater than 7.
Acids react with salts to produce a base and water.
A solution has a pH of 5. Which type of solution does this represent?
Acidic
Basic
Neutral
None of these are true
The table below shows data from an investigation designed to find a liquid that is both a base and a strong electrolyte.
Solution 1
Solution 2
Solution 3
Solution 4
Two clear solutions are placed in separate beakers. The first solution has a pH of 4 and the second solution has an unknown pH. When the two solutions are mixed together, the resulting pH is 5. What must be true of the second solution?
Fewer suspended solids
A lower temperature
More dissolved acid (HCl) particles
A higher concentration of OH⁻ ions
Which of the following is NOT a strong electrolyte?
HCl
HNO₃
H₂SO₄
HCOOH
