Unit 2 Set 2 (Water Chemistry)
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70 Terms
What is an Arrhenius acid?
A substance that increases the concentration of H⁺ or H₃O⁺ in aqueous solution.
What is an Arrhenius base?
A substance that increases the concentration of OH⁻ in aqueous solution.
What is a Brønsted-Lowry acid?
A proton donor.
What is a Brønsted-Lowry base?
A proton acceptor.
What is a Lewis acid?
An electron-pair acceptor.
What is a Lewis base?
An electron-pair donor.
What is an amphiprotic substance?
A substance that can either donate or accept a proton.
Why is H₂O amphiprotic?
It can accept H⁺ to form H₃O⁺ or donate H⁺ to form OH⁻.
Is HCl an acid or a base?
Acid.
Is HNO₃ an acid or a base?
Acid.
Is H₂SO₄ an acid or a base?
Acid.
Is HClO₄ an acid or a base?
Acid.
Is NH₃ an acid or a base?
Base.
Is OH⁻ an acid or a base?
Base.
Is H₃O⁺ an acid or a base?
Acid.
Is NH₄⁺ an acid or a base?
Acid.
Is CH₃COO⁻ an acid or a base?
Base.
Is CO₃²⁻ an acid or a base?
Base.
Is HCO₃⁻ an acid, a base, or both?
Both. It is amphiprotic.
Is HSO₄⁻ an acid, a base, or both?
Both. It can donate or accept H⁺.
Is BH₃ a Lewis acid or Lewis base?
Lewis acid.
Is NH₃ a Lewis acid or Lewis base?
Lewis base.
In HCl + H₂O → H₃O⁺ + Cl⁻, what is HCl?
Acid.
In HCl + H₂O → H₃O⁺ + Cl⁻, what is H₂O?
Base.
In HCl + H₂O → H₃O⁺ + Cl⁻, what is Cl⁻?
Conjugate base.
In HCl + H₂O → H₃O⁺ + Cl⁻, what is H₃O⁺?
Conjugate acid.
In NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, what is NH₃?
Base.
In NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, what is H₂O?
Acid.
In NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, what is NH₄⁺?
Conjugate acid.
In NH₃ + H₂O ⇌ NH₄⁺ + OH⁻, what is OH⁻?
Conjugate base.
In HCN + OH⁻ → CN⁻ + H₂O, what is HCN?
Acid.
In HCN + OH⁻ → CN⁻ + H₂O, what is OH⁻?
Base.
In HCN + OH⁻ → CN⁻ + H₂O, what is CN⁻?
Conjugate base.
In HCN + OH⁻ → CN⁻ + H₂O, what is H₂O?
Conjugate acid.
What is the conjugate base of HCl?
Cl⁻.
What is the conjugate base of HNO₃?
NO₃⁻.
What is the conjugate base of H₂SO₄?
HSO₄⁻.
What is the conjugate base of HSO₄⁻?
SO₄²⁻.
What is the conjugate base of H₂O?
OH⁻.
What is the conjugate base of HCO₃⁻?
CO₃²⁻.
What is the conjugate acid of NH₃?
NH₄⁺.
What is the conjugate acid of OH⁻?
H₂O.
What is the conjugate acid of CO₃²⁻?
HCO₃⁻.
What is the conjugate acid of HCO₃⁻?
H₂CO₃.
How do members of a conjugate acid-base pair differ?
By exactly one H⁺.
HCl is what type of acid?
Strong acid, hydrochloric acid.
HBr is what type of acid?
Strong acid, hydrobromic acid.
HI is what type of acid?
Strong acid, hydroiodic acid.
HNO₃ is what type of acid?
Strong acid, nitric acid.
H₂SO₄ is what type of acid?
Strong acid, sulfuric acid.
HClO₃ is what type of acid?
Strong acid, chloric acid.
HClO₄ is what type of acid?
Strong acid, perchloric acid.
LiOH is what type of base?
Strong base, lithium hydroxide.
NaOH is what type of base?
Strong base, sodium hydroxide.
KOH is what type of base?
Strong base, potassium hydroxide.
RbOH is what type of base?
Strong base, rubidium hydroxide.
Ba(OH)₂ is what type of base?
Strong base, barium hydroxide.
Sr(OH)₂ is what type of base?
Strong base, strontium hydroxide.
What is the autoionization reaction of water?
2 H₂O ⇌ H₃O⁺ + OH⁻.
What is the expression for Kᵥ?
Kᵥ = [H⁺][OH⁻].
What is Kᵥ at 25°C?
1.0 × 10⁻¹⁴.
What must always be true for neutral water?
[H⁺] = [OH⁻].
Does neutral water always have a pH of 7?
No. Neutral means [H⁺] = [OH⁻].
At 25°C, what is the pH of neutral water?
7.
What happens to Kᵥ as temperature increases?
Kᵥ increases.
What happens to the pH of neutral water as temperature increases?
It decreases.
Is neutral water with a pH below 7 acidic?
No. It is neutral if [H⁺] = [OH⁻].
What is the equation for pH?
pH = −log[H⁺].
What is the equation for pOH?
pOH = −log[OH⁻].
At 25°C, what is the relationship between pH and pOH?
pH + pOH = 14.