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NEUTRALIZATION NOTES
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1. Neutralization means:
Moles acid [H+] = moles of base [OH-]
VOCABULARY
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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
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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
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burette
Standard solution, a solution
of known [M]
Analyte, a solution of
unknown [M]
ring stand
burette
clamp
(indicator)
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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)
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VOCABULARY
4. End point: point in titration where the indicator
changes color to signal the equivalence point
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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
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MAVAnA = MBVBnB
M= molarity V= volume (L, mL, etc.) nA= #H
+ n
B= #OH
-
Acid
Base
TITRATION CALCULATIONS
(see Formulas)
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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
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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
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