NEUTRALIZATION NOTES

1. Neutralization means:

Moles acid [H+] = moles of base [OH-]

VOCABULARY

A NEUTRALIZATION REACTION IS A REACTION BETWEEN

AN ACID AND BASE TO PRODUCE A SALT AND WATER.

HCl + NaOH NaCl + H2O

salt* + water

*A salt is any compound containing the cation

from a base and anion from an acid

Acid + Base

VOCABULARY

2. A titration is a laboratory method used to

determine the concentration of an acid or base

(analyte) in a solution by performing a

neutralization reaction with a titrant (standard).

Standard: one you know the concentration [M] of

burette

Standard solution, a solution

of known [M]

Analyte, a solution of

unknown [M]

ring stand

burette

clamp

(indicator)

VOCABULARY

3. The titrant is added to the analyte until the

Equivalence point is reached. This is the point

when H+ ions equal OH

- ions (Neutralization)

VOCABULARY

4. End point: point in titration where the indicator

changes color to signal the equivalence point

STRONG ACID + STRONG BASE

• STRONG ACID + STRONG BASE

TITRATIONS: EQUIVALENCE

POINT IS ALWAYS PH 7

• WANT AN INDICATOR THAT HAS

AN ENDPOINT CLOSE TO THE

EQUIVALENCE POINT

MAVAnA = MBVBnB

M= molarity V= volume (L, mL, etc.) nA= #H

+ n

B= #OH

-

Acid

Base

TITRATION CALCULATIONS

(see Formulas)

MAVAnA = MBVBnB

Write

Eq’n

Ex 1: If 42.5 mL of 1.3 M KOH are used to neutralize

50.0 mL of H2SO

4, find the molarity of H

2SO

4.

KOH +

H

2SO

4 K

2SO

4 +

H

2O

2

2

If 42.5 ml of 1.3M KOH are used to neutralize

50.0 ml of H2SO4, find the molarity of H2SO4.

H+ (acid)

H2SO4

VA = 50.0 mL

MA= ?

nA = 2

OH- (base)

KOH

VB = 42.5 mL

MB = 1.3 M

nB = 1

MAVAnA = MBVBnB

VAnA VAnA

MA= 1.3 M x 42.5 mL x 1

50.0 mL x 2

MA= 0.55 M

MAVAnA = MBVBnB