Last Unit

Molarity

………..Mols((Solute)…………………………………………………………………………………………….M L(solution)

molality

………..Mols((Solute)…………………………………………………………………………………………….m kg(solvent-whatever there’s more of)

why can’t polar dissolve into nonpolar

like dissolves like

polar dissolves polar

if temp in solid goes up-

more solute can be dissolved

if temp in a gas goes up

it can hold less

Binary acids

H and one other element (hydrochloric acid)

Oxyacids

H + compound

ATE IC ITE OUS

car batteries

sulfuric acid

explosives

Nitric Acid

fertilizers

phosphoric Acids

pepsi/coke

phosphoric acid

stomach

hydrochloric acid

vinegar

acetic acid

sour milk

lactic acid

properties of acids

Sour taste

Produce hydronium H3O+ ions

Change the color of acid-base indicators

React with active metals to release hydrogen gas

React with bases to produce salts and water

Conduct electric current

Common Properties of Bases

Taste bitter

Produce hydroxide OH- ions

Change the color of acid-base indicators

Feel slippery

React with acids to produce salts and water

Conduct electric current

Arrhenius Acids and Bases

Arrhenius acid - increases H+ ions (H3O+)

Arrhenius base - increases OH- ions

Weak acid

weak electrolyte (end in -COOH)

strong acid

ionizes completely, strong electrolyte (ex. HCl)

Alkaline

base completely dissociates in water to yield OH- ions

Strong bases

completely dissociates, strong electrolyte (end in OH)

Bronsted Lowry

Bronsted-Lowry Acid - proton donor

Bronsted-Lowry Base - proton acceptor

Monoprotic acid

donates one proton HCl

Diprotic acid

donates two protons H2SO4

Triprotic acid

donates three protons H3PO4

Conjugate Acids and Bases

Conjugate base - the species that remains after a Bronsted-Lowry acid has given up a proton

Conjugate acid - the species that is formed when a Bronsted-Lowry base gains a proton

Strength of Acid/Conj. Base

Strong acid🡪weak conjugate base

Weak acid🡪strong conjugate base

Amphoteric compound

any species that can react as either an acid or a base

Neutralization

the reaction of hydronium ions and hydroxide ions to form water molecules and salt Self-ionization of water

H3O+ + OH- 🡪2H2O or H2O + H2O🡪H3O+ + OH-

Self-ionization of water

H3O + OH ←→H2O + H2O

Buffers

A solution that resists a change in its pH even when a strong acid or base is added to it.

A solution is buffered by the presence of a weak acid and its conjugate base.

Added H+ reacts with base

Added OH- reacts with weak acid

lye

sodium hydroixde

milk of magnesia

magnisum hydroxide

antacids

almunium hydroxide