Aqueous Equilibria Key Terms

effect on equilibrium when a substance with an ion in common with the dissolved species is added to the solution; causes a decrease in the solubility of an ionic species, or a decrease in the ionization of a weak acid or base

• common ion effect

• coupled equilibria

• selective precipitation

• titration curve

mixture of appreciable amounts of a weak acid-base pair the pH of a buffer resists change when small amounts of acid or base are added

• buffer capacity

• buffer

• molar solubility

• titration curve

amount of an acid or base that can be added to a volume of a buffer solution before its pH changes significantly (usually by one pH unit)

• buffer

• Henderson-Hasselbalch equation

• buffer capacity

• coupled equilibria

system characterized the simultaneous establishment of two or more equilibrium reactions sharing one or more reactant or product

• selective precipitation

• common ion effect

• solubility product constant (K_sp)

• coupled equilibria

logarithmic version of the acid ionization constant expression, conveniently formatted for calculating the pH of buffer solutions

• selective precipitation

• Henderson-Hasselbalch equation

• solubility product constant (K_sp)

• buffer

solubility of a compound expressed in units of moles per liter (mol/L)

• solubility product constant (K_sp)

• molar solubility

• selective precipitation

• buffer

process in which ions are separated using differences in their solubility with a given precipitating reagent

• selective precipitation

• buffer

• coupled equilibria

• Henderson-Hasselbalch equation

equilibrium constant for the dissolution of an ionic compound

• titration curve

• solubility product constant (K_sp)

• buffer capacity

• buffer

plot of some sample property (such as pH) versus volume of added titrant

• coupled equilibria

• titration curve

• buffer capacity

• buffer