Chemistry Chap 8:acids And Bases And Oxidation-Reduction

Front 1

Arrhenius Theory of Acids & Bases

Back 1

According to this theory, an acid, dissolved in water, dissociates to form hydrogen ions or protons (H+), and a base, dissolved in water, dissociates to form hydroxide ions (OH-).

Some substances have acid or base properties but can not be explained using the Arrhenius Theory.

Front 2

Properties of Acids:

Back 2

-sour taste
-corrosive
-will react with many metals to produce hydrogen gas
-will neutralize bases (react with bases to produce water and a salt)
-will change the color of acid-base indicators (litmus paper turns pink or red in acids; phenolphthalein is colorless in acids)

Front 3

Properties of Bases

Back 3

-bitter taste
-caustic
-slippery feeling
-will neutralize acids (react with bases to produce water and a salt)
-will change the color of acid-base indicators (litmus paper turns blue in bases; phenolphthalein is pink to magenta in acids)

Front 4

Neutralization Reaction:

Back 4

The hydrogen ion of the acid combines with the hydroxide ion of the base to form water; the cation of the base and the anion of the acid form an aqueous solution (usually the salt is soluble in water) of an ionic compound which is called a salt

Front 5

Bronsted-Lowry Theory of Acids & Bases

Back 5

-broadens the view of acids and bases and can explain why these substances are acids or bases.
An acid as a proton (H+) donor and a base as a proton acceptor.

-the acid donates a proton to a base; the acid by donating the proton becomes a base; the base by accepting the proton becomes an acid.

Hint 5

notes and 241

Front 6

The acid and the base it forms when it donates the proton is called a conjugate acid-base pair

Back 6

-a conjugate acid is what is formed when a base accepts a proton
-a conjugate base is what is formed when an acid donates a proton

Front 7

amphiprotic

Back 7

a substance that can behave either as a Bronsted acid or a Bronsted base.

Example water