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WorksheetsExploring Acids and Bases
Total questions: 15
Worksheet time: 8mins
What is the Bronsted-Lowry definition of an acid?
A Bronsted-Lowry acid is a proton donor.
A Bronsted-Lowry acid is a compound that does not react with water.
A Bronsted-Lowry acid is a substance that increases hydroxide ions in solution.
A Bronsted-Lowry acid is a base that accepts protons.
What is the Bronsted-Lowry definition of a base?
A Bronsted-Lowry base is a substance that increases acidity.
A Bronsted-Lowry base is a neutral molecule that does not react with protons.
A Bronsted-Lowry base is a proton donor.
A Bronsted-Lowry base is a proton acceptor.
Identify the conjugate acid of NH3.
NH2-
N2H4
NH3O+
NH4+
Identify the conjugate base of H2O.
OH-
O2-
H3O+
H2O2
Which of the following is a strong acid: HCl, CH3COOH, or H2CO3?
NH3
H2SO4
HCl
NaOH
Which of the following is a weak base: NaOH, K2CO3, or NH4OH?
NH4OH
NaOH
K2CO3
HCl
What is the conjugate acid of HSO4-?
H2SO3
H2S
HSO3-
H2SO4
What happens to the pH of a solution when a strong acid is added?
The pH of the solution increases.
The pH of the solution remains the same.
The pH of the solution decreases.
The pH of the solution fluctuates randomly.
Write the balanced equation for the neutralization of HCl with NaOH.
HCl + NaOH → Na2O + H2
HCl + NaOH → NaCl + O2
HCl + KOH → KCl + H2O
HCl + NaOH → NaCl + H2O
What is the conjugate base of H2SO4?
HSO4-
HSO3-
H2SO3
H2SO5
How do you determine the strength of an acid?
The strength of an acid is based on its temperature.
The strength of an acid is measured by its viscosity.
The strength of an acid is determined by its pH level, dissociation constant (Ka), and titration results.
The strength of an acid is determined by its color.
What is the result of mixing equal moles of a strong acid and a strong base?
A solution that produces gas when mixed.
The result is a neutral solution (pH ~ 7) of water and salt.
A highly acidic solution with a pH below 3.
A highly basic solution with a pH above 11.
What is the pH of a neutral solution at 25°C?
6
7
8
5
Identify the conjugate acid-base pair in the reaction: H2O + NH3 ⇌ NH4+ + OH-.
(NH4+, NH3) and (H2O, OH-)
(NH4+, H2O)
(OH-, NH3)
(H2O, NH4+)
Explain the role of water in the Bronsted-Lowry acid-base theory.
Water can act as both an acid and a base in the Bronsted-Lowry theory.
Water can only act as an acid in the Bronsted-Lowry theory.
Water is not involved in acid-base reactions according to Bronsted-Lowry.
Water can only act as a base in the Bronsted-Lowry theory.
