Acids and bases Flashcards
Define the term strong acid. (L.C)
An acid that fully dissociates in solution and is a good proton donor.
Define the term dibasic acid. (L.C)
A dibasic acid produces two H⁺ ions in solution e.g. H₂SO₄.
Define acid (Bronsted-Lowry theory) (L.C)
An acid is a proton (H⁺) donor.
Define conjugate pair (Bronsted-Lowry theory) (L.C)
Two substances that differ by one proton.
What is the conjugate base of nitric acid :
4HNO₃ → 2H₂O + 4NO₂ + O₂ (L.C)
NO₃-
Define acid according to the Bronsted-Lowry theory.(L.C)
An acid is a proton (H⁺) donor.
Define base according to the Bronsted-Lowry theory . (L.C)
A base is a proton (H⁺) acceptor.
Identify the acid, and conjugate acid in the following system: H₂S + O²- ⇾ OH- + SH- (L.C)
H₂S (both are acids and both are conjugate bases)
OH-
Write (i) the conjugate acid and (ii) the conjugate base of HPO₄²-. (L.C)
Conjugate acid - H₂PO₄-
Conjugate base - PO₄³-
Identify one species acting as an acid, and also identify its conjugate base in the following system : H₂F⁺ + Cl- ⇌ HCl + HF
(must match correct one)
Acid - H₂F⁺ / HCl
Conjugate base - HF / Cl-
Distinguish between a strong acid and a weak acid. (L.C)
Strong acid - an ad that fully dissociates in solution and is a good proton donor.
Weak acid - an acid that is a poor proton donor and only slightly dissociated in solution.
Distinguish between a strong acid and a weak acid. (L.C)
Strong acid - an ad that fully dissociates in solution and is a good proton donor.
Weak acid - an acid that is a poor proton donor and only slightly dissociated in solution.
Define acid according to the theory of Bronsted-Lowry. (L.C)
An acid is a proton (H⁺) donor.
Distinguish between a strong acid and a weak acid. (L.C)
Strong acid - an acid that fully dissociates in solution and is a good proton donor.
Weak acid - an acid that is a poor proton donor and only slightly dissociated in solution.
Identify the two conjugate pairs in the following dissociation of nitrous acid (HNO₂): HNO₂ + H₂O ⇌ NO₂- + H₃O⁺
- HNO₂ and NO₂-
- H₂O and H₃O⁺
Define acid according to the Bronsted-Lowry theory. (L.C)
An acid is a proton (H⁺) donor.
Define conjugate acid according to the Bronsted-Lowry theory. (L.C)
A base plus a H⁺ ion.
Distinguish between a strong acid and a weak acid. (L.C)
Strong acid - an acid that fully dissociates in solution and is a good proton donor.
Weak acid - an acid that is a poor proton donor and only slightly dissociated in solution.
Define an acid in terms of the Bronsted-Lowry theory. (L.C)
An acid is a proton (H⁺) donor.
What is a conjugate pair? (L.C)
Two substances that differ by one proton.
How do strong acids differ from weak acids in their behaviour in water according to the Arrhenius’ theory. (L.C)
Strong : Almost completely dissociated to give hydrogen ions (H⁺) in solution.
Weak : Only slightly dissociated to give hydrogen ions (H⁺) in solution.
What is the conjugate base of (i) sulfuric acid, (ii) the weak acid of HA? Which of these conjugate bases is stronger? Explain (L.C) MORE XOXO
(i) HSO₄-
(ii) A-
(iii) A-
(iv) Conjugate base of a weak acid.
Explain, by giving a balanced equation for its dissociation in water, that the conjugate base of sulfuric acid is itself an acid. (L.C)
HSO₄- + H₂O ⇾ SO₄²- + H₃O⁺
How do strong acids differ from weak acids in their behaviour in water according to the Bronsted-Lowry theory. (L.C)
Strong : good proton (H⁺) donor.
Weak : poor proton (H⁺) donor
