### Classwork
06 August 2024
### Conjugate Acid-Base Pairs
#### Part 1: Classification as Bronsted-Lowry Acid, Base, or Both
1. Cl^-
- Classification: Base
- Explanation: Chloride ion (Cl^-) is the conjugate base of hydrochloric acid (HCl). It has the ability to accept a proton (H^+), thus acting as a base.
2. HSO3^-
- Classification: Both
- Explanation: Bisulfite ion (HSO3^-) can act as both an acid and a base. It can donate a proton to become SO3^2- or accept a proton to become H2SO3.
3. HCOOH
- Classification: Acid
- Explanation: Formic acid (HCOOH) is a typical acid. It can donate a proton to become HCOO^-.
4. HSO4^-
- Classification: Both
- Explanation: Bisulfate ion (HSO4^-) can act both as an acid and a base. It can donate a proton to become SO4^2- or accept a proton to become H2SO4.
5. H2O
- Classification: Both
- Explanation: Water (H2O) is amphoteric, meaning it can act both as an acid and a base. It can donate a proton to become OH^- or accept a proton to become H3O^+.
6. H3O^+
- Classification: Acid
- Explanation: Hydronium ion (H3O^+) is a proton donor and thus classified as an acid.
#### Part 2: Conjugate Acids
1. H3PO4
- Conjugate Acid: H4PO4^+
- Explanation: The conjugate acid of H3PO4 (phosphoric acid) is obtained by adding a proton (H^+) to it, resulting in H4PO4^+.
2. H2PO4^-
- Conjugate Acid: H3PO4
- Explanation: The conjugate acid of H2PO4^- (dihydrogen phosphate ion) is H3PO4 (phosphoric acid) formed by accepting a proton.
3. HS^-
- Conjugate Acid: H2S
- Explanation: The conjugate acid of HS^- (hydrosulfide ion) is H2S (hydrogen sulfide) obtained by accepting a proton.
4. NO3^-
- Conjugate Acid: HNO3
- Explanation: The conjugate acid of NO3^- (nitrate ion) is HNO3 (nitric acid) formed by accepting a proton.
#### Summary
- Classifications:
- Cl^-: Base
- HSO3^-: Both
- HCOOH: Acid
- HSO4^-: Both
- H2O: Both
- H3O^+: Acid
- Conjugate Acids:
- H3PO4: H4PO4^+
- H2PO4^-: H3PO4
- HS^-: H2S
- NO3^-: HNO3
