Acids and Bases
- Created by: Leanne Baker
- Created on: 24-02-14 13:51
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- ACIDS AND BASES
- Bronsted-Lowry Acids and Bases
- Acid = Proton donor
- Base = Proton acceptor
- Acid-base equilibria = transfer of protons
- pH of Strong Acids
- pH = -Log10[H+]
- [H+] = 10-pH
- pH of Strong Bases
- Ionic Product of Water
- Water is weakly dissociated
- Kw = [H+][OH-]
- [H+] = Kw/[OH-]
- pH of Strong Bases
- Ionic Product of Water
- Water is weakly dissociated
- Kw = [H+][OH-]
- [H+] = Kw/[OH-]
- Water is weakly dissociated
- Ionic Product of Water
- pH of Strong Bases
- Water is weakly dissociated
- Ionic Product of Water
- Buffer Solutions
- Resists changes in pH when small amounts of acid or alkali are added, or when it is diluted
- At an equilibrium
- pH of buffer solutions
- [H+] = Ka[acid]/[salt]
- pH = pKa x Log10([salt]/[acid])
- Resists changes in pH when small amounts of acid or alkali are added, or when it is diluted
- pH Curves
- Titration Calculations
- Strong acid, strong base
- -Calculate number of moles of H+ ions and OH- ions in each solution -Work out which ion is in excess -Calculate the total volume of the mixture -Calculate the concentration of the excess ion -Calculate pH
- Weak acid, strong base
- -Calculate number of moles of weak acid and OH- ions in each solution -Work out which one is in excess -Calculate the total volume of the mixture -Calculate [H+] and pH from excess ions
- Strong acid, strong base
- pH of Weak Acids
- Weak acids and bases only dissociate slightly in aqueous solution
- Ka = [H+][A-]/[HA]
- For a weak acid in aqueous solution, [H+] = [A-]
- So Ka = [H+][H+]/[HA]
- Ka = Acid dissociation constant
- For a weak acid in aqueous solution, [H+] = [A-]
- pKa = -Log10Ka
- Bronsted-Lowry Acids and Bases
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