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Page 1: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode
Page 2: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Acids are electrolytes that:

Produce H+ (as H3O+) ions in water – always listed

first in the formula

Turn blue litmus red

Taste sour

Corrode metals

Neutralizes bases to form salts and water

Low pH (1-6)

Page 3: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Examples of Acids

• Vinegar Acetic acid

• Carbonated Drinks Carbonic acid

• Vitamin C Ascorbic acid

Page 4: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Bases are electrolytes that:

Produce OH- ions in water

Taste bitter

Burns skin (caustic)

Feel soapy, slippery

Neutralizes acids to form salts and water

High pH (8 – 14)

Turns litmus paper blue

Page 5: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Examples of BasesExamples of Bases

• Soaps

• Ammonia Cleaner

• Drain cleaners

• Baking soda

• Lye

• Tums - antacids

Page 6: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Litmus paper tests

Blue litmus paper turns red in acids

Red litmus paper turns blue in bases

Page 7: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

When an acid combines with a base, a When an acid combines with a base, a neutralization reaction occurs making neutralization reaction occurs making

salt plus water.salt plus water.

Acid + Base --- Salt + Water

Negative ions of acid combine with Positive ions of base.

Example: HCl + NaOH -- NaCl + H2O

http://www.photoghetto.com/photos/water/39.htm
http://0.tqn.com/d/chemistry/1/0/E/S/1/salt-crystals.jpg
Page 8: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Characteristics of SaltCharacteristics of Salt

• pH of 7

• pH hydrion paper turns green

• Is an electrolyte in solution (can conduct an electric current)

• Evaporate salt water solution, salt crystals will form

• MANY different kinds of salts

• Magnesium sulfate salt

Page 9: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Strengths of acids and basesStrengths of acids and bases Strong electrolytes are completely

dissociated into ions in water. Weak acids

and bases do not completely ionize. • Strong acids completely

dissociate in water, forming H+ and an anion. There are six strong acids. The others are considered to be weak acids.

• HCl - hydrochloric acid • HNO3 - nitric acid • H2SO4 - sulfuric acid

• Strong bases dissociate 100% into the cation and OH- (hydroxide ion). The hydroxides of the Group I and Group II metals usually are considered to be strong bases.

• LiOH - lithium hydroxide • NaOH - sodium hydroxide • KOH - potassium

hydroxide

Page 10: Acids are electrolytes that: þ Produce H + (as H 3 O + ) ions in water – always listed first in the formula þ Turn blue litmus red þ Taste sour þ Corrode

Dilute vs. ConcentratedDilute vs. Concentrated

• To dilute an acid or a base, you add water.

• You can dilute a strong acid, HCl by adding water. 10 ml of HCl plus:

* 100 ml of water, it is concentrated.

-It is a concentrated, strong acid.

* 1000ml of water, it is dilute.

-It is a dilute, strong acid.


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