CHAPTER 14ACIDS AND BASES

14.1PROPERTIES OF ACIDS AND BASES

14.1A practical application of acids and bases.

These two flowers are exactly the same genus and species, so why are they different colors?

14.1A practical application of acids and bases.

These two flowers are exactly the same genus and species, so why are they different colors?

It is the pH of the soil they are grown in.

14.1What are some properties of acids?

14.1What are some properties of acids? Sour taste (commonly found in foods) Change the color of pH indicators Most react with active metals to produce H2

React with bases to produce water and a salt (neutralization reaction)

Conduct electricity

14.1Naming acids

Binary acids – hydrogen and one other element“hydro_________ic acid”

Oxyacids – hydrogen, oxygen, and one other element“per_________ic acid” per -________-ate“_________ic acid” ________-ate“_________ous acid” ________-ite“hypo_________ous acid” hypo_________-ite

14.1Example 1: Name the following:

H3PO4

HBr

HClO3

HClO2

H2SO4

HC2H3O2 or CH3COOH

HI

HNO3

14.1Common industrial acids

sulfuric – H2SO4

most commonly produced chemical in the worldmetallurgy, fertilizers, petroleum refining, dehydrating

agent, car batteriesnitric – HNO3

explosives, plastics, pharmaceuticalsphosphoric – H3PO4

fertilizers, animal feed, flavoring in food, detergentshydrochloric – HCl

cleaning metals and masonry, swimming pool acid, stomach acid

acetic – CH3COOH

plastics, food supplements, fungicidecarbonic – H2 CO3

carbonation in sodas

PH OF SOME COMMON SUBSTANCES

14.1What are some properties of bases?

14.1What are some properties of bases? Taste bitter Change the color of pH indicators Feel slippery React with acids to produce water and a salt Conduct electricity

14.1Naming bases

Use ionic naming rules for –OH and other ionic bases. Some have common names (NH3).

14.1Common bases

NaOH – oven cleaner, lyeCaO – “lime” on lawns, cement, mortarNH3 - ammonia, cleaner, dissolved in water is NH4OH

Al(OH)3, Mg(OH)2, and NaHCO3 – antacids

NaHCO3 – baking soda

14.1What determines a “strong” base or acid?

14.1The strength of acids and bases is based on how easily they

form ions in solution.

14.1The strength of acids and bases is based on how easily they

form ions in solution.

STRONG ACID

WEAK ACID

When the strong acid ionizes, what is the result?

When the weak acid ionizes, what is the result?

Why would this be important?

14.1The strength of acids and bases is based on how easily they

form ions in solution.

A strong acid forms lots of H3O1+, a weak acid forms few H3O1+

A strong base forms lots of OH1-, a weak base forms few OH1-

Do not confuse strength with a high concentration. A strong acid could be in a very dilute solution, and a weak acid could be in a very concentrated solution.

14.1

Without counting ions or measuring conductivity, how could strength be determined?

14.1The arrow holds the key.

Strong acidHNO3 + H2O H3O+ + NO3

1-

Weak acidHCN + H2O H3O+ + CN1-

Strong baseNaOH Na+ + OH1-

Weak baseNH4OH NH4

+ + OH1-

14.1Example 2: Show dissociation of these strong bases and

ionization of these strong acids when added to water 

Mg(OH)2

14.1Example 2: Show dissociation of these strong bases and

ionization of these strong acids when added to water 

HClO3 + H2O

14.1Example 2: Show dissociation of these strong bases and

ionization of these strong acids when added to water 

NaOH

14.1Example 2: Show dissociation of these strong bases and

ionization of these strong acids when added to water H2SO4 + H2O

14.1Example 3: Show ionization of these weak bases and acids

when added to water HCN + H2O

14.1Example 3: Show ionization of these weak bases and acids

when added to water NH3 + H2O

14.1Example 3: Show ionization of these weak bases and acids

when added to water H3PO4 + H2O

14.1Example 3: Show ionization of these weak bases and acids

when added to water HCO3

1- + H2O

acting as a base

14.1