| A | B |
|---|
| common ion | A charged species consisting of a metal ion surrounded by ligands. |
| common ion effect | The shift in an equilibrium position caused by the addition or presence of an ion involved in the equilibrium reaction. |
| buffered solution | A solution that resists a change in its pH when either hydroxide ions or protons are added. |
| Henderson-Hasselbalch equation | An equation giving the relationship between the pH or an acid-base system and the concentrations of base and acid. |
| buffering capacity | The abiity of a buffered solution to absorb protons or hydroxide ions without a significant change in pH; determined by the magnitudes of [HA] and [A-] in the solution |
| solubility product constant | solubility product- the constant for the equilibrium expression representing the dissolving of an ionic solid in water. |
| millimole | mmol- a thousandth of a mole. |
| equivalence point | stoichiometric point- The point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated. |
| acid-base indicator | A substance that marks the end point of an acid-base titration by changing color. |
| phenolphthalein | A commonly used indicator, colorless in its HIn acid form and pink in its In- or basic form. |
| pH curve | titration curve- A plot showing the pH of a solution being analyzed as a function of the amount of titrant added. |
