Chemistry - Acids and Bases

Know the common industrial acid known as muriatic acid.

Know the common industrial acid known as muriatic acid.

HCl (hydrochloric acid)

Know the acid manufactured in the largest amount.

H2SO4 (Sulfuric acid)

Be able to choose the strongest base from a list of compounds.

H2O, NaOH, NH3, HCl

NaOH is the strongest. The reason? OH- is hydroxide ions, making bases stronger.

In a given reaction be able to identify the conjugate acid-base.

EX: HF + H2O > F- + H3O

HF is the acid

H2O is the base

F- is the conjugate base

H3O is the conjugate acid

The stronger an acid is, the (stronger/weaker) its conjugate base.

The stronger a base, the (stronger/weaker) its conjugate acid.

weaker, weaker. Remember: it’s always inverse

Acid strength (increases/decreases) with (increasing/decreasing) polarity and (increasing/decreasing) bond strength.

increases, increasing, decreasing

Acid + Base > ? + ?

Acid + Base > water + salt

If you have barium carbonate + HCl > ? + ?

barium chloride + carbon dioxide

diprotic

donates 2 protons

binary

2 acids mixed together (hydrogen + something with electro negativity)

When an acids donates a proton, it becomes a

conjugate base

It can be an acid or a base (ex: H2O)

amphoteric

HBrO

hypobromous acid

HI

hydroiodic acid

H2SO4

sulfuric acid

H2CO3

carbonic acid

HCl

hydrochloric acid

HNO2

nitrous acid

hydrosulfuric acid

H2S

perchloric acid

HCLO4

phosphorous acid

H3PO3

nitric acid

HNO3

List the conjugate acid and base pairs. Identify each reactant + product as an acid or a base.

HF + H2O > F- + H3O

PAIRS:

HF + F-

H2O + H3O

ACID OR BASE:

HF + F- = acidic

H2O + H3O = basic

List the conjugate acid and base pairs. Identify each reactant and product as a proton donor or acceptor.

H2O + NH3 > NH4 + OH-

PAIRS:

H2O + OH-

NH3 + NH4

DONORS AND ACCEPTORS:

H2O + OH- = donors

NH3 + NH4 = acceptors

Acid Base Neutralization formula equation

HCL + NaOH > NaCL + H2O

Acid Base Neutralization overall net ionic equation

H3O+ + CL- + Na+ + OH- > Na+ + Cl- + 2H2O

Acid base Neutralization net ionic equation

H3O+ + OH- > 2H2O

periodic acid

HIO4

iodic acid

HIO3

hypoiodous acid

HIO

List HIO4, HIO3, HIO from weakest to strongest

HIO, HIO3, HIO4

Explain the difference between strong acids and weak acids

Any acid that fully dissociates into ions is strong, if it doesn’t it’s weak

Explain how the production of sulfur trioxide, SO3, in industrial processes results in acid rain. Write an equation for the reaction.

SO3 produces as a gas. It dissolves in the water vapor in the clouds. This produces sulfuric acid solution that falls like rain or snow.

SO3 + H2O > H2SO4

List five properties of aqueous acids

Sour taste

change in color of acid-base indicator

some react with metal to release hydrogen gas

react w/ bases to produce salt and H2O

conduct electric current

Write the balance equations that describe the three stage ionization of phosphoric acid in a dilute aqueous solution

1. H3PO4 + H2O > H3O + H2PO4

2. H2PO4 + H2O > H3O + HPO4 2-

3. HPO4 2- + H2O > H3O PO4 3-