Classwork
06 August 2024
Conjugate Acid-Base Pairs

1. Classify the following as Bronsted-Lowry acid, base, or both.
1. [tex]Cl^{-}[/tex]
2. [tex]HSO_3^{-}[/tex]
3. HCOOH
4. [tex]HSO_4^{-}[/tex]
5. [tex]H_2O[/tex]
6. [tex]H_3O^{+}[/tex]

2. Write the conjugate acid for the following:
- [tex]H_3PO_4[/tex] → [tex]H_2PO_4^{-}[/tex]
- [tex]HS^{-}[/tex]
- [tex]NO_3^{-}[/tex]

Question

06-08-2024
Chemistry

Answered

Classwork
06 August 2024
Conjugate Acid-Base Pairs

1. Classify the following as Bronsted-Lowry acid, base, or both.
1. [tex]Cl^{-}[/tex]
2. [tex]HSO_3^{-}[/tex]
3. HCOOH
4. [tex]HSO_4^{-}[/tex]
5. [tex]H_2O[/tex]
6. [tex]H_3O^{+}[/tex]

2. Write the conjugate acid for the following:
- [tex]H_3PO_4[/tex] → [tex]H_2PO_4^{-}[/tex]
- [tex]HS^{-}[/tex]
- [tex]NO_3^{-}[/tex]

Answer :

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GinnyAnswer GinnyAnswer · Answer 1 · 2024-08-06T15:27:15-04:00

### 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