ACIDS and BASES

Properties of Acids

Properties of Bases

Naming Acids and Bases

For Acids We can use Table K to help us with naming

Acids are polar covalent and will give off hydrogen ions

Two types of acids exist

Binary Acids

Contain Hydrogen and 1 other (non-metal) element

All Binary acids begin with the prefix HYDROAll Binary acids end with –ic acidExample:HCl will be named:HYDROchlorIC acid

Ternary Acids

Give away H+ ions when dissolved in waterFeature Oxygen containing polyatomic ions

with Hydrogen NO3 SO4

If the Polyatomic ends with (ate) we call this an IC ACID

Example: H2SO4SO4 = SulfateSo Acid is Sulfuric Acid

Naming Continued

If the polyatomic ends with ITE we name this an OUS acid.

Example:H2SO3 Would be named: Sulfurous Acid Notice that in all cases NO HYDRO is used to

name a ternary acid. Most can be found in Table K

Naming Bases

Steps to Follow

Bases are usually ionic compounds (Metal and non-metal) that release OH- ions in solution.

Consist of a group 1 or 2 metal with hydroxide Therefore we just follow regular naming rules

for ionic compounds when naming mostNaOH consists of sodium and hydroxideName: Sodium HydroxideMetal keeps its name, and polyatomic OH ions

keep theirs as well. Table L gives a list of common bases and names

The Nature of the Hydrogen Ion

Has No Electron when it is ionized (H+)So it looks for something to bind to for

stabilityIn water it attaches itself to the water

molecule and forms an H3O+ ion (hydronium)

Creates an ion complex with acid like properties

This is why you can indicate the presence of an acid with either the H+ ion or the H3O+ ion

Illustration of Hydronium Ion

Nature of the Hydroxide Ion

OH- is what makes many bases basicGiven off when a basic compound is placed

into waterThe more OH- (hydroxide ions) that you

release in water, the stronger you are in terms of base strength (higher pH 10-14)

If H+ ions are present, OH- ions will bind with it to form water (basis of neutralization)