The student will:

understand the concept of acids/bases.

will identify from a reaction strong/weak acid/base.

will be able to explain dissociation or ionization and its relationship to strength of acid/base.

Will be able to identify a monoprotic, diprotic, triprotic acid.

will be able to compare/ contrast pH of liquids

no ws

Acids Vs. Base

What do lemons and pickles taste like?

What does soap feel like?

Acids & Bases do the same thing except from opposite directions

Acids taste sourLemon, oranges, grapefruit = citric acidYogurt, sour milk = lactic acidCarbonated drinks = carbonic acidVinegar = acetic acid

Bases taste bitterSoap = bitterShell of nuts = bitter

Acids & Bases

6 acidsSulfuric H2SO4

Nitric HNO3

Hydrochloric HCl

Phosphoric H3PO4

Carbonic H2CO3

Acetic Acid HC2H3O2

What do you notice?

What makes an acid an acid?

BasesSodium Hydroxide NaOH

Magnesium Hydroxide Mg(OH)2

Aluminum Hydroxide Al(OH)3

Potassium Hydroxide KOH

Calcium Hydroxide Ca(OH)2

Barium Hydroxide Ba(OH)2

What do you notice?What makes a base a base? (OH) or the ability to make an (OH)

Ammonia NH3

Sodium Hydrogen Carbonate NaHCO3

Base solutions are sometimes called ALKALINE SOLUTIONS

Back to AcidsBack to Acids

HCl + H20 H+ + Cl-

Acids … ionize themselves… break apart into their ions.

Remember water is very polar

HCl + H20 H30+ + Cl-

You may see…either….. H30+ or H+

These have names:

Hydronium ion, hydrogen ion, proton ion

Back to BasesBack to Bases

Bases dissociate ….. Break apart producing hydroxide

NaOH + H20 Na+ + OH-

NH3 + H20 NH4+ + OH-

Which ion accounts for the alkalinity of bases in water solutions?

1. Hydronium ion

2. Sodium ions

3. Hydroxide ions

4. Alkali metals

Which of the following is an alkali?

1. Mg(OH)2

2. H2SO4

3. HCl

4. ZnCO3

Before

ionization

After

ionization

Contents of solution

Strong Acid

HAcid H+ A-

Weak Acid

HAcid H+ W

H+ B-

Strong vs. Weak

Can tell 2 ways memorize them arrows

Strong acids: HCl, H2SO4, HNO3 ionize completely

Weak acids: H2CO3, HC2H3O2, H3PO4

Strong Base: group 1, 2 metals dissociates completely

Weak base: NH3

HF + H20 F- + H30+

H2SO4 + H20 HSO4 + H30+

Strength of acids

depends on: H+ production

polarity of bonds

ionization

The greater the polarity of bond = greater strength

The greater the ionization = greater strengthThe ease with which the hydrogen to the element bond can be broken

Strong acids= HCl, HNO3, H2SO4

Weak Acid = H3PO4, H2CO3, HC2H3O2

Notice: strength of acid does not depend on number of hydrogens

Strength of bases depends on: OH- production

polarity of bonds

dissociation of hydroxide

Base solutions are sometimes called

alkaline solutions

Strong Bases: NaOH, KOH, Ca(OH)2, Ba(OH)2

Weak Base: NH3

According to the dissociation theory, the ion present in all basic

solutions is…

1. O-2

2. OH-

3. H3O-1

4. OH-2

The term strong and weak refer to…

1. The concentration of the electrolyte.

2. The degree of ionization

3. The amount of solvent

4. The number of electron pairs

5. The number of hydrogens

Monoprotic

Diprotic

Triprotic

HCl, H2SO4, HNO3

H3PO4, H2CO3, HC2H3O2

Return to strength of Acid/Base

Memorize list -- look at arrows -- measure the pH.

What makes an Acid an Acid?

What makes a base a base?

Pure water is neutral

pH = 7

“self- ionizes”

Water molecule + water molecule = hydronium ion + hydroxide ion

Neutral because equal number of hydronium and hydroxide( ½ ½ )

H30+

OH-

pH scale

Power of the hydrogen

pH scale measures:the concentration of the hydromium ion or hydroxide ion.

pH = 0…..14

0 3 7 10 14

Units of 10

Ph paper/ instruments

The will student will:

understand the concept of acids/bases

will identify from a reaction strong/weak acid/base

will be able to explain dissociation or ionization and its relationship to its strength.

Will be able to identify a monoprotic, diprotic, triprotic acid

will be able to compare/contrast pH of liquids

no ws