Chapter 18: Aqueous Ionic Equilibriums

solvent definition

dissolving thing

solute

dissolved thing

liquids soluble in each other =

miscible

liquids not soluble in each other =

immiscible

unsaturated solution description

not reached limit of solute that will dissolve, no solid on bottom of container

saturate solution description

the minimum amount of dissolved solute at a given temp, SOLID ON THE BOTTOM

supersaturated descriptions

more solute than a saturated solution will hold at that temp, very unstable, tricks the solution, no solid either

solubility-product constant

Ksp

saturated is a keyword that means what

means equilibrium has been reached

5% Rule

if x < 5% of the initial concentration it can be ignored in ICE calculations

the solubility of a slightly soluble salt _____ when a common ion is added (product ion)

decreases bc equilibrium shifts left to offset the increase

how does pH affect solubility (only works for solutions with OH- and F- ions)

add a strong acid so that the OH- and the H+ form water, so the equilibrium shifts left and more of the salt dissolves

why does this only work with strong acids?

strong acids split apart while weak acids do not

what are the 7 strong acids?

HBr, HCl, HI, HNO3, H2SO4, HClO4, HClO3

how does formation of complex ions affect solubility?

if complex ions are formed from ions of a slightly soluble salt, the equilibrium will continue to shift left until the entire solid has dissolved

what is a ligand?

central atom in complex ions i think

Amphoteric oxides and bases…

cannot dissolve in neutral water but can in strongly acidic or basic solutions

they are complex anions with hydroxides bonded

If Q > Ksp…

precipitation occurs until Q = Ksp

If Q = Ksp…

equilibrium exists

Q < Ksp

solid dissolves until Q = Ksp

selective precipitation definition

when ions are separated from each other due to the solubilities of their salts (difference in K values)