Ap chem

What are the (Arrhenius) strong acids?

completely disassociate in water + increase h+ concentration:

HCl (Hydrochloric acid)

HNO3 (Nitric acid)

H2SO4 (sulfuric acid)

HBr (hydroponic acid)

HI (Hydroiodic acid)

HClO4 (Perchloric acid)

HClO3 (chloric acid)

What are the (Arrhenius) strong bases

A compound that completely ionizes in water + increase OH- concentration:

• Potassium hydroxide (KOH)

• Sodium hydroxide (NaOH)

• Barium hydroxide (Ba(OH)2)

• Caesium hydroxide (CsOH)

• Strontium hydroxide (Sr(OH)2)

• Calcium hydroxide (Ca(OH)2)

• Lithium hydroxide (LiOH)

• Rubidium hydroxide (RbOH)

How are Bronsted-Lowry acids/bases different from Arrhenius acids/bases?

Bronsted-Lowry concept extends to any molecule (not just OH- and H+) or substance, where an (Bronsted-Lowry) acid is a proton donor and a base is a proton acceptor.

How is a Lewis acid/base different from an Arrhenius acid/base?

Lewis acids/bases revolve around electrons, instead of protons.

-Lewis acids: receive electrons (yes receive)

-Lewis bases: donate electrons

Amphiprotic

A substance capable of acting as either an acid or a base

Ex. H2O can turn into OH- or H3O+

Conjugate base

A base formed by removing the proton from an acid

OH- is the conjugate base of H2O

Conjugate Acid

Acid formed by adding a proton to the base

H3O+ is the conjugate acid of H2O

Conjugate Acid-base pair

When an acid donates a proton, it becomes a base. When a base receives a proton, it becomes an acid.

Polyprotic acids/bases

Acids that are capable of losing more than a single proton in an acid-base reaction/Acids that have more than one ionizable H+ atom.

Ex. H2SO4

Bases that can receive more than one proton in a acid-base reaction

Ex. PO4³-

Acid dissociation constant + base dissociation constant

Ka; greater Ka =stronger acid.

Kb, larger = stronger base:

When will [H] = [OH]

At the equivalent point

What is a buffer?

A solution with a stable pH; adding an acid or a base doesn’t greatly affect the pH (Unless it is a big amount). Formed by adding a weak acid/base and its conjugate:

How do we calculate pH of a buffer?

The Henderson-Hasselbalch Equation