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Jun 5
There are three types of basicity of an acid:
1. Monobasic acid: An acid that can donate only one proton per molecule is called a monobasic acid. Examples include hydrochloric acid (HCl) and nitric acid (HNO3).
2. Dibasic acid: An acid that can donate two protons per molecule is called a dibasic acid. Examples include sulfuric acid (H2SO4) and carbonic acid (H2CO3).
3. Tribasic acid: An acid that can donate three protons per molecule is called a tribasic acid. An example is phosphoric acid (H3PO4).
1. Monobasic acid: An acid that can donate only one proton per molecule is called a monobasic acid. Examples include hydrochloric acid (HCl) and nitric acid (HNO3).
2. Dibasic acid: An acid that can donate two protons per molecule is called a dibasic acid. Examples include sulfuric acid (H2SO4) and carbonic acid (H2CO3).
3. Tribasic acid: An acid that can donate three protons per molecule is called a tribasic acid. An example is phosphoric acid (H3PO4).
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Google Gemini AI
Jun 5
1. Arrhenius Basicity:
- Definition: The ability of an acid to donate H+ ions in an aqueous solution, resulting in an increase in H+ ion concentration.
- Measurement: Equivalence point in acid-base titration.
- Examples: HCl, H2SO4, HNO3
2. Brønsted-Lowry Basicity:
- Definition: The ability of an acid to donate a proton (H+) to a base.
- Measurement: Strength of the conjugate base.
- Examples: Acetic acid (CH3COOH), carbonic acid (H2CO3), phosphoric acid (H3PO4)
3. Lewis Basicity:
- Definition: The ability of an acid to accept an electron pair from a base.
- Measurement: Affinity for electron pairs.
- Examples: BF3, AlCl3, H+
4. Carboxylic Acid Basicity:
- Definition: The ability of a carboxylic acid to donate a hydrogen ion from the carboxylic acid group (-COOH).
- Measurement: Ka (acid dissociation constant).
- Examples: Acetic acid (pKa = 4.76), benzoic acid (pKa = 4.20)
5. Phenolic Acid Basicity:
- Definition: The ability of a phenolic acid to donate a hydrogen ion from the hydroxyl group (-OH) attached to the aromatic ring.
- Measurement: Ka (acid dissociation constant).
- Examples: Phenol (pKa = 10.00), salicylic acid (pKa = 2.97)
- Definition: The ability of an acid to donate H+ ions in an aqueous solution, resulting in an increase in H+ ion concentration.
- Measurement: Equivalence point in acid-base titration.
- Examples: HCl, H2SO4, HNO3
2. Brønsted-Lowry Basicity:
- Definition: The ability of an acid to donate a proton (H+) to a base.
- Measurement: Strength of the conjugate base.
- Examples: Acetic acid (CH3COOH), carbonic acid (H2CO3), phosphoric acid (H3PO4)
3. Lewis Basicity:
- Definition: The ability of an acid to accept an electron pair from a base.
- Measurement: Affinity for electron pairs.
- Examples: BF3, AlCl3, H+
4. Carboxylic Acid Basicity:
- Definition: The ability of a carboxylic acid to donate a hydrogen ion from the carboxylic acid group (-COOH).
- Measurement: Ka (acid dissociation constant).
- Examples: Acetic acid (pKa = 4.76), benzoic acid (pKa = 4.20)
5. Phenolic Acid Basicity:
- Definition: The ability of a phenolic acid to donate a hydrogen ion from the hydroxyl group (-OH) attached to the aromatic ring.
- Measurement: Ka (acid dissociation constant).
- Examples: Phenol (pKa = 10.00), salicylic acid (pKa = 2.97)
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