Acids: liberate H+ ions in solution.Bases: liberate OH- ions in solution.

Arrhenius Definitions:

An acid-base reaction in which water is formed is called a neutralization.

Acids: proton donors

Bases: proton acceptors

Brӧnsted- Lowry Definitions:

What volume of 0.20 M NaOH must be added to 25.0 mL of 0.15 M HC2H3O2 to neutralize the acid?

25.0 mL acetic acid

1

0.15 mol

1000.0mL 1 mole acetic acid

1 mole NaOH 1000.0 mL

0.20 mol NaOH

=19 mL NaOH

Volume of acid present

Molarity of acid

Mole ratioUpside down molarity of base…1/Mb

= volume of base needed

MaVa =(1/Mb) Vb MaVa= MbVb

What volume of 0.20 M NaOH must be added to 25.0 mL of 0.15 M HC2H3O2 to neutralize the acid?

25.0 mL acetic acid

1

0.15 mol

1000.0mL 1 mole acetic acid

1 mole NaOH 1000.0 mL

0.20 mol NaOH

= 19 mL NaOH

Volume of acid present

Molarity of acid

Mole ratioUpside down molarity of base…1/Mb

= volume of base needed

MaVa =(1/Mb) Vb MaVa= MbVb

Ba(OH)2

Ba(OH)2

2

Ba(OH)2

9.4 mLBa(OH)2

2(If base has 2 hydroxides/formula)

MaVa = MbVb (for one to one mole ratio neutralizations)

MaVa = 2MbVb (for neutralizations involving bases with 2

hydoxides per FU)2MaVa = MbVb (for neutralizations involving diprotic

acids)

What is the molarity of an H2SO4 solution if a volume of 22.3 mL of LiOH (with a concentration of 0.75 M) is needed to neutralize 100.0 mL of it?

2MaVa = MbVb

2Ma(100.0 mL) = (0.75 M)(22.3mL)

Ma = 0.084 M