WorksheetsChemistry Quiz on Acids and Bases
Total questions: 40
Worksheet time: 20mins
What is the pH of a 0.0025 M solution of hydrochloric acid?
2.6
7.0
1.2
A BrØnsted-Lowry base is defined as a substance that ___.
increases [H+] when placed in H2O
Decrease [H+] when placed in H2O
increase [OH-] when placed in H2O
acts as a proton acceptor
acts as a proton donor
What is the conjugate base of OH-?
O2
O-
O2-
H2O+
H2O
A substance that is capable of acting as both an acid and as a base is _______.
saturated
Autosoma
miscible
amphoteric
Conjugated
A BrØnsted-Lowry acid is defined as a substance that _______.
acts as a proton acceptor
decrease [H+] when placed in H2O
increase [H+] when placed in H2O
acts as a proton donor
Increases [OH-] when placed in H2O
What is the conjugate acid of NH3?
NH4OH
NH2+
NH4+
NH3
NH2+
What is the expression for the ion-product constant of water (Kw) at 25°C?
Kw = [H₃O⁺] / [OH⁻]
Kw = [H₃O⁺] × [OH⁻]
Kw = [H₂O]²
Kw = [H⁺] + [OH⁻]
In pure water at 25°C, what are the concentrations of H₃O⁺ and OH⁻ ions?
[H₃O⁺] = 1.0 × 10⁻⁷ M; [OH⁻] = 1.0 × 10⁻⁷ M
[H₃O⁺] = 1.0 × 10⁻⁶ M; [OH⁻] = 1.0 × 10⁻⁸ M
[H₃O⁺] = 1.0 × 10⁻⁸ M; [OH⁻] = 1.0 × 10⁻⁶ M
[H₃O⁺] = 1.0 × 10⁻¹⁴ M; [OH⁻] = 1.0 M
What does it mean when a substance is described as amphoteric?
It can only donate protons.
It can only accept protons.
It can act as both an acid and a base.
It is neutral and does not participate in acid-base reactions.
If the concentration of H₃O⁺ in a solution is 1.0 × 10⁻⁵ M at 25°C, what is the concentration of OH⁻?
1.0 × 10⁻⁵ M
1.0 × 10⁻⁹ M
1.0 × 10⁻⁷ M
1.0 × 10⁻¹⁴ M
What is the pH of pure water at 25°C?
0
7
14
It varies depending on atmospheric pressure.
What is the pH of an aqueous solution at 25 *C that contains 3.98 x 10^-9 M hydronium?
8.40
5.60
9.00
3.98
7.00
Calculate the pOH of a solution at 25 *C that contains 1.94 x 10^-10 M hydronium ions?
1.94
4.29
7.00
14.0
9.71
What is the pH of an aqueous solution at 25 *C that contains 3.98 x 10^-9 hydroxide ion?
8.40
5.60
9.00
3.98
7.00
What is the concentration (in M) of hydroxide ions in a solution at 25 *C with pH= 4.282.
4.28
9.72
1.92 x 10^-10
5.22 x 10^-5
1.66 x 10^4
What is the concentration of hydronium ions in a solution at 25 *C with a pH= 4.282
4.28
9.72
1.92 x 10^-10
5.22 x 10^-5
1.66 x 10^4
Which is one of the seven strong acids?
HClO4
NAOH
KOH
Which one is not a strong base?
NaOH
KOH
HNO3
The most common soluble strong bases are…
Ionic hydroxides of alkali metals
Partially ionized in aqueous solution
Composed entirely of carbon, hydrogen, and oxygen
What is the concentration of a 0.0011 M Ca(OH)2 solution in water?
0.0011 M
0.0022 M
0.0012 M
What is the pH of Ca(OH)2 in water?
11.34
11.43
9.2
What is the formula for percent ionization?
(Initial HA / H⁺ equilibrium) × 100%
(Ka × HA) × 100%
(H⁺ equilibrium / Initial HA) × 100%
(HA² / H₂O) × 100%
What is the Ka expression for CH₃COOH?
[CH₃COOH] / [H⁺][CH₃COO⁻]
[H⁺][CH₃COO⁻] / [CH₃COOH]
[H₂O] × [CH₃COOH]
[CH₃COOH] × [CH₃COO⁻]
If a 0.035 M solution of HNO₂ produces 3.7 × 10⁻³ M of H⁺, what is its percent ionization?
5%
11%
20%
2%
What does a smaller Ka value indicate about a weak acid?
It ionizes less
It is stronger
It is a base
It forms a precipitate
What is the general formula for the ionization of a weak acid HA in water?
HA + H₂O ⇌ H₃O⁺ + A⁻
H₂O ⇌ H⁺ + OH⁻
HA ⇌ H₂ + A
H₂O + A⁻ ⇌ HA + OH⁻
A solution of ammonia has a molarity of 0.1M and a Kb 1.8x10^-5. What is the hydroxide ion concentration?
1.3x10^-3
9.4x10^-7
8.2x10^-3
9.6x10^-4
Find the hydroxide ion concentration for 0.05 M of some base with a Kb of 4.8x10^-4.
1.6x10^-3
4.9x10^-3
5.9x10^-3
2.8x10^-6
A 0.2 M solution of some base has a Kb of 1.7x10^-9 find the hydronium ion concentration
6.0x10^-11
9.2x10^-3
5.4x10^-10
8.9x10^-2
What is the pH of a 0.8 M solution with a Kb of 5.0x10^-9.
7
5
11
9.8
The Ka of an unknown acid is 4.9 x 10^-10. What is the value of Kb for the acid?
3.9 x 10^-26
2.0 x 10^-5
4.9 x 10^-4
2.9 x 10^-17
The acid-dissociation constant, Ka for Gallic acid is 5.52 x 10^-4. What is the base-dissociation constant, Kb, for the gallate ion?
4.57 x 10^-3
2.19 x 10^-12
1.8 x 10^-11
3.4 x 10^-7
Ka for HF is 7.0 x 10^-4. Kb for the fluoride ion is ______.
2.0 x 10^-8
1.4 x 10^-11
7.0 x 10^-18
3.5 x 10^-5
What is the pKa of some acid that has a Ka of 6.5 x 10^-5?
6.7 x 10^-6
2.8
4.0 x 10^-4
4.2
What is the pKb of some acid that has Ka of 3.3 x 10^-9
5.5
7.3
3.8
6.2
What determines whether an anion will affect the pH of an aqueous solution?
Strength of the anion's conjugate acid
strength of the anion's conjugate base
strength of the anion's acid
strength of the anion's base
Explain why the chloride ion (Cl-) is considered a spectator ion in acid-base chemistry.
It’s a base, which means it will react with nothing
It’s a acid, which means it reacts with water to be a spectator
It's a conjugate acid is strong, and has a tendency to react with water to produce (OH-)
It's a conjugate acid is strong, and has a tendency to react with water to produce (OH-)
Predict whether an aqueous solution of sodium acetate (CH3COONa) will be acidic, basic, or neutral.
Basic
Neutral
Strong
Weak
What is hydrolysis.
Type of musical genre that combines water sounds with techno beats
A reaction with nothing, meaning no acid-base reaction
A substance reacts with water to produce either H+(aq) or OH-(aq)
When water molecules are converted into hydrogen gas and oxygen without any energy input.
A salt solution is prepared by dissolving potassium fluoride (KF) in water. Will the resulting solution be acidic, basic, or neutral?
Basic
Neutral
Strong
Weak
