Terms : Hide Images
| 8399359397 | pH | Is the amount hydrogen ions (H+) or hydronium ion (H3O+) In water. Acidic (H+), base (OH-) | 0 | |
| 8399428539 | Equilibrium constant | K=[Products]/[Reactants] | 1 | |
| 8399453860 | Water is amphoteric | Amphoteric means that is donates hydrogen ions in acids and accepts Hydrogen ions in bases. | 2 | |
| 8399496099 | Conjugate Acid | it is a base with a hydrogen ion added to it, accepted hydrogen ion | 3 | |
| 8399541549 | Conjugate base | it is an acid with a hydrogen ion removed from it, donated Hydrogen ion | 4 | |
| 8399612529 | Weak acid Same base | Ka<1 | 5 | |
| 8399639893 | Strong acid Same base | Ka>1 | 6 | |
| 8399654146 | Strong acids | HCl (hydrochloric acid), HBr (Hydrobromic acid), HI ( hydroiodic acid), HClO3(chloric acid), H2SO4(sulfuric acid ),HNO3(Nitric acid) | 7 | |
| 8400035865 | pKa | is a measure of acid strength pKa=-log Ka | 8 | |
| 8400102628 | Buffer | is a solution made of acid and its Conjugate base to resist drastic change in pH or base and its conjugate acid | 9 | |
| 8400160613 | Henderson-hasselbalch equation | pH=pKa+ log [CB/A] ... CB: Conjugate base, A:Acid Or this can be written as pH=pKa- log [A/CB] |  | 10 |
| 8400353965 | Ka | is a quantitative measure of the strength of an acid in solution. Higher Ka means stronger acid | 11 | |
| 8400552872 | Why use buffers? | To mimic biological systems pH for experimental systems, such as blood pH at 7.4 or other organism/proteins that need specific pH to function at. | 12 | |
| 8401066359 | Kw | Ionisation constant of water Kw= K[H2O] = [H+][OH-] = 10^-14 | 13 | |
| 8412549149 | Acid | Have a higher Hydrogen concentration therefore stronger acids would have higher Ka. It also have less OH- ions | 14 | |
| 8412612443 | Base | Have a lower hydrogen concentration therefore stronger bases would have higher Kb. it also has more OH- ions. | 15 |
