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WorksheetsAcid-Base Equilibria Quiz
Total questions: 31
Worksheet time: 16mins
What is the definition of an acid according to the Brønsted-Lowry theory?
A substance that donates electrons
A substance that accepts protons
A substance that donates protons
A substance that produces hydroxide ions
What is the pH of a neutral solution at 25°C?
0
7
14
10
What is the definition of a base according to the Brønsted-Lowry theory?
A substance that donates protons
A substance that accepts protons
A substance that produces hydrogen ions
A substance that produces hydroxide ions
Which of the following is a strong base?
Sodium bicarbonate
Ammonium hydroxide
Sodium hydroxide
Calcium carbonate
Which statement about amphoteric substances is true?
They can only act as acids.
They can only act as bases.
They can act as both acids and bases.
They do not participate in acid-base reactions.
Which of the following statements about pH is true?
pH = -log[H⁺]
pH = log[H⁺]
pH = [H⁺]
pH = 10^[-H⁺]
What is Kw at 25°C?
1.0 × 10⁻¹⁴
1.0 × 10⁻¹²
1.0 × 10⁻¹⁶
1.0 × 10⁻¹³
Which of the following is a characteristic of a strong acid?
It partially ionizes in solution.
It completely ionizes in solution.
It has a high pKa value.
It has a low conductivity in solution.
In a reaction between an acid and a base, what is produced?
Salt and water
Hydrogen gas and salt
Acid and base
Oxide and water
What happens to the equilibrium position when you increase the temperature of an exothermic reaction?
It shifts to the right (products).
It shifts to the left (reactants).
It remains unchanged.
It shifts randomly.
Which ion is responsible for acidic properties in aqueous solutions?
OH⁻
H⁺ (or H₃O⁺)
Na⁺
Cl⁻
What type of reaction occurs when an acid reacts with a carbonate?
Neutralization reaction
Redox reaction
Decomposition reaction
Precipitation reaction
Which of the following acids is considered weak?
HCl
HNO₃
CH₃COOH (acetic acid)
H₂SO₄
In which type of solution would you expect to find a higher concentration of hydroxide ions (OH⁻)?
Acidic solution
Neutral solution
Basic solution
Saturated solution
What happens to the pH of a solution when a strong acid is added to it?
The pH increases.
The pH decreases.
The pH remains constant.
The pH becomes neutral.
Which equation represents the dissociation of water?
H_2O ⇌ H^+ + OH^-
H_2O + OH^- → H_2O_2 + e^-
H_2O → H_2 + O_2 + heat
H_2O + NaCl → NaOH + HCl
What is the formula for calculating the pKa from Ka?
pKa = log(Ka)
pKa = -log(Ka)
pKa = Ka / 10
pKa = 10^(-Ka)
What happens to the equilibrium position when an acid is added to a buffer solution?
It shifts to produce more acid.
It shifts to produce more base.
It remains unchanged.
It shifts to produce water.
What is the conjugate base of HCl?
Cl⁻
H₃O⁺
H₂Cl⁺
Cl₂
What is the relationship between Ka and Kb for a conjugate acid-base pair?
Ka + Kb = Kw
Ka × Kb = Kw
Ka / Kb = Kw
Ka = Kb
Which of the following is a strong acid?
Acetic acid
Hydrochloric acid
Carbonic acid
Phosphoric acid
Which of the following factors affects the strength of an acid?
The number of hydrogen atoms in the molecule.
The electronegativity of atoms bonded to hydrogen.
The molecular weight of the acid.
The color of the acid.
What happens to the concentration of hydronium ions when you add a strong base to a solution?
It increases.
It decreases.
It remains constant.
It fluctuates randomly.
What is the purpose of a buffer solution?
To change the pH dramatically
To maintain a stable pH when small amounts of acid or base are added
To neutralize acids only
To increase the concentration of hydrogen ions
Which indicator would you use to determine the endpoint of a strong acid-strong base titration?
Phenolphthalein
Methyl orange
Bromothymol blue
Litmus paper
Which of the following would act as a Lewis acid?
H₂O
NH₃
BF₃
CH₃COOH
In a buffer solution, what components are typically present?
Strong acid and strong base
Weak acid and its conjugate base
Strong acid and its conjugate base
Weak base and its conjugate acid
What is the primary component of a buffer solution made from acetic acid and sodium acetate?
Strong acid and strong base
Weak acid and its salt (conjugate base)
Strong base and weak acid
Weak base and its salt (conjugate acid)
Which of the following statements about weak acids is true?
They completely dissociate in solution.
They have high conductivity in solution.
They only partially dissociate in solution.
They have low pKa values.
What is the effect of dilution on the pH of a strong acid?
The pH increases.
The pH decreases.
The pH remains constant.
The pH becomes neutral.
What is the conjugate acid of NH₃?
NH₂⁻
NH₄⁺
N₂H₄
H₂N₂
