Strong Acids and Bases

Hydrochloric Acid

HCl is a strong acid

Sulfuric Acid

H2SO4 is a strong acid. It is made of the sulfate ion and hydrogen.

Nitric Acid

HNO3 is a strong acid. It is made of the nitrate ion and hydrogen.

Hydrobromic acid

HBr is a strong acid

Hydroiodic acid

HI is a strong acid

perchloric acid

HClO4 is a strong acid. It is made of the perchlorate ion and hydrogen.

Sodium Hydroxide

NaOH is a strong BASE

Acetic Acid (Vinegar)

HC2H3O2 is a weak acid. It is made of the acetate ion and a hydrogen.

Lithium hydroxide

LiOH is a strong base

Potassium hydroxide

KOH is a strong base

Calcium Hydroxide

Ca(OH)2 is a strong base

Strontium hydroxide is a strong base

Sr(OH)2

Barium hydroxide is a strong base

Ba(OH)2

Strong acids ionize

completely

Weak acids ionize

only a little

Strong acids have a large

Ka value because there are many more products than reactants

Weak acids have small

Ka values because there are few products and more reactants.

NH_3 (Ammonia) is a

Bronsted Lowry Base. It accepts a proton to become ammonium NH4+.

All Bronsted Lowry Bases are

Lewis Bases.

All Arrhenius Acids are

Bronsted Lowry acids

NOT all Lewis Acids are

Bronsted Lowry acids or Arrhenius acids.

Arrhenius acids have these at the front and are aqueous. They release these.

H+

Arrhenius bases release

hydroxide ions. OH-

Bronsted Lowry acids are

proton donors.

Bronsted Lowry bases are

proton acceptors

Lewis acids are

electron acceptors

Lewis bases are

electron donors

Salts are made from the

anion of the acid and the cation of the base

What is the salt created from Ba(OH)2 and H2SO4?

BaSO4 -- This is barium sulfate.

What is the salt created from KOH and H3PO4?

K3PO4 - remember to put charges on top and swap and drop! PO4 has a charge of -3. K has a charge of +1.

Using MaVa = MbVb what does Ma stand for?

molarity of the acid

MaVa = MbVb. What does Vb stand for?

Volume of the base.

The equivalence point is

the point in a titration where the number of moles of hydrogen ions equals the number of moles of hydroxide ions

The end point

the point in a titration at which an indicator changes color

Acids turn litmus paper

red

Bases turn litmus paper

blue

a pH below 7 indicates:

excess of h+ ions, and an acidic solution

a pH above 7 indicates:

base

percent dissociation

Amount dissociated M / initial concentration M x 100%

Hydronium ion formula

Hydroxide ion