Weak acid
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Acid-base reaction theories pH Self-ionization of water Buffer solutions Systematic naming Electrochemistry Acids: Bases: |
[\mathrm \, \leftrightarrow \, H^+\,_ +\, A^-\,_ }]
The equilibrium concentrations of reactants and products are related by the Acidity constant expression, (Ka):
[\mathrm }]
The greater the value of Ka, the more the formation of H+ is favored, and the lower the pH of the solution. The Ka of weak acids varies between 1.8×10-16 and 55.5. Acids with a Ka less than 1.8×10-16 are weaker acids than water. Acids with a Ka of greater than 55.5 are strong acids and almost totally dissociate when dissolved in water.
The vast majority of acids are weak acids.
Weak Acid Ionisers
- Phosphoric acid, H3PO4
- Ethanoic acid, CH3COOH
- Hydrofluoric acid, HF
- Acetylsalicylic acid, C6H4OCOCH3CO2H
- Nicotinic acid, C5H5NCOOH
- Pyruvic acid, CH3COCOOH
- Bromothymol blue, C21H15NaBr2O3S
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