Solubility Equilibria

solvent/solute

solute is dissolved in the solvent

saturated

maximum amount of solute is dissolved in a solvent

unsaturated

less than the maximum amount of solute is dissolved in a solvent

supersaturated

more than the maximum amount of solute is dissolved in a solvent

large Ksp

most soluble

smallest Ksp

least soluble

lewis acid

electron acceptorle

lewis base

electron donor

chelating agent

multi-denate ligands make many bonds to metal ions and can

“sequester” them

acidic salts

more soluble in basic solutions and less soluble in acidic solutions

basic salts

more soluble in acidic solutions and less soluble in basic conditions

neutral salts

Solubility is independent of pH

negligible cations

group 1 metals

group 2 metals

M+ (metals with +1 charge)

All others are acidic

more + charged, more acidic

negligible anions

Cl-

Br-

I-

NO₃^-

ClO₄^-

ClO₃^-

all others are basic

HSO₄^- IS ACIDIC

van’t hoff factor (i)

The number of ions a compound dissociates into per formula unit

Raoult’s Law

vapor pressure depression - partial pressure of a volatile solute above a solution

Boiling point elevation

highest boiling point - highest molality

freezing point depression

highest freezing point = lowest molal

colligative properties

1. Vapor pressure depression

2. boiling point elevation

3. freezing point depression

4. osmotic pressure

5. Henry’s Law

Henry’s Law

solubility of a gas in solution

bronsted- lowry acid

H+ donor

bronsted-lowry base

H+ acceptor

amphoteric

describes a substance that can act as both an acid and a base

amphiprotic

describes a substance that can act as both a proton (H+) donor or acceptor

HClO₄

strong acid

H₂SO₄

strong acid

HI

strong acid

HBr

strong acid

HCl

strong acid

HNO₃

strong acid

HClO₃

strong acid

group 1 metals

strong bases

hydroxides

strong bases

Ba(OH)₂

strong base

Sr(OH)₂

strong base

Ca(OH)₂

strong base

Mg(OH)₂

strong base

buffers

resists changes in pH

made from weak conjugate acid/conjugate base pair

strong acid/base titration curve

pH equivalence point ~7

weak acid/strong base

pH equivalence point >7

weak base/strong acid

pH equivalence point <7

bromcresol green

pka - 4.8 - turns solution green

bromothymol blue

pka - 7.1 — turns the solution blue

phenolphthalein

pka- - 9.7, will turn the solution pink

half equivalence point

pKa - half protonated and deprotonated

equivalence point

pH - all deprotonated