Chapter 17: Bronsted-Lowry Acid Base Theory + Strong and Weak Acids

Which pair is not a conjugate acid-base pair?

a. (CH3)3N; (CH3)3NH+

b. H2SO4; H2SO3

c. HNO2; NO2

b. H2SO4; H2SO3

Brønsted-Lowry acids are H+ _______.

donors

Brønsted-Lowry bases are H+ __________.

acceptors

____________________ can act as either an acid or a base because they have both a transferable H and an atom with lone pair electrons.

Amphoteric substances

Conjugate acid-base pairs differ by ______________

one proton (one H+ ion)

Strong acids donate practically all of their

H+ ions

Weak acids donate

a small fraction of their H+ ions

The smaller ionization constant, K, the weaker the

base

The farther the equilibrium position lies toward the products,

the stronger the acid or base.

Commonly, acid or base strength is measured by

determining the equilibrium constant of a substance's reaction with water.

The stronger an acid is at donating H,

the weaker the conjugate base is at accepting H.

Higher oxidation number =

stronger oxyacid

Trend in base strength is

opposite of acid strength.

larger Ka =

stronger acid

Ka=

[H30+][A-]/HA= [H+][A-]/HA