Acids and Bases: Brønsted–Lowry Acid–Base Equilibria in Aqueous Solution Flashcards
What are Brønsted–Lowry acids?
- Proton (H+) donors
What are Brønsted–Lowry bases?
- Proton (H+) acceptors
Give the general equation for the reaction between acids and water
- HA (aq) + H2O (l) → H3O+ (aq) + A- (aq)
- Acid (HA) donates protons to water
What is the H3O+ ion called?
- Hydroxonium ion
Give the general equation for the reaction between bases and water
- B (aq) + H2O (l) → BH+ (aq) + OH- (aq)
- Base (B) accepts proton from water
What do acids and bases do in water?
- Dissociate
- Break up into positively and negatively charged ions
How much do strong acids dissociate in water?
- Fully dissociate
- HX + water → H+ (aq) + X- (aq)
Give examples of strong acids
- Hydrochloric acid
- Sulfuric acid
- Nitric acid
How much do weak acids dissociate in water?
- Slightly dissociate
- HA + water ⇌ H+ (aq) + A- (aq)
Give examples of weak acids
- Organic acids like ethanol
- Ethanoic acid
- Citric acid
How much do strong bases dissociate in water?
- Fully dissociate
- B + water → B+ (aq) + OH- (aq)
Give an example of a strong base
- Sodium hydroxide
How much do weak bases dissociate in water?
- Slightly dissociate
- B + water ⇌ B+(aq) + OH- (aq)
Give an example of a weak base
- Ammonia
The reactions of strong bases/acids with water are reversible. Why are only the forward reactions shown?
- The equilibrium lies far to the right so only forward reaction shown
- HA + water ⇌ H+ (aq) + A- (aq)
- B + water → B+ (aq) + OH- (aq)
