1950164
| Question | Answer |
| equation for pH | - log [H+] |
| How to work out [H+] from pH | 10 ^ -pH |
| Bronsted - Lowry Acid Definition | A proton donor |
| Bronsted - Lowry Base Definition | A proton acceptor |
| Strong Acid Definition | An acid which completely dissociates in aqueous solution |
| Weak Acid Definition | An acid which only partially dissociates in aqueous solution |
| Ka (Acid Dissociation Constant) | |
| Units for Ka | mol dm ^ -3 |
| A large Ka indicates what? | A large extent of dissociation, therefore the acid is strong |
| A small Ka indicates what? | A small extent of dissociation, therefore the acid is weak |
| equation for pKa | |
| How to work out Ka from pKa | 10 ^ -pKa |
| The smaller the value of pKa ... | ... the stronger the acid |
| equation for Kw (ionic product of water) | [H+] x [OH-] |
| At 25 degree Celsius, the value of Kw is | 1.00 x 10 ^ -14 |
| Units for Kw | mol ^ 2 dm ^ -3 |
| Buffer Definition | A mixture which minimises pH changes on the addition of small amounts of acid or base |
| What is an acidic buffer solution made of? | A weak acid and a salt of the weak acid e.g ethanoic acid and sodium ethanoate |
| What is an alkaline buffer solution made of? | A weak base and a salt of the weak base e.g ammonia and ammonium chloride |
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