This document discusses acid-base titration, including definitions of acids and bases, strong vs weak acids and bases, and the technique of titration. It explains that a titration reaches the equivalence point when the moles of acid equals the moles of base, producing a neutral solution. This can be shown using the equation MAVA = MBVB, where M is molarity, V is volume, and A and B indicate acid and base. An example titration calculation is provided.

1. ACID BASE TITRATION
HENNI FITRIANI
8136141004

2. Acid & Base
Acids:
acids are sour tasting
Arrhenius acid: Any substance that, when dissolved in
water, increases the concentration of hydronium ion
(H3O+)
Bronsted-Lowry acid: A proton donor
Lewis acid: An electron acceptor
Bases:
bases are bitter tasting and slippery
Arrhenius base: Any substance that, when dissolved in
water, increases the concentration of hydroxide ion (OH-)
Bronsted-Lowery base: A proton acceptor
Lewis acid: An electron donor

3. Introduce Of Acid

4. Introduce Of Base

5. Example
STRONG vs WEAK
_ completely ionized _ partially ionized
_ strong electrolyte _ weak electrolyte
_ ionic/very polar bonds _ some covalent bonds
Strong Acids: Strong Bases:
HClO4 LiOH
H2SO4 NaOH
HI KOH
HBr Ca(OH)2
HCl Sr(OH)2
HNO3 Ba(OH)2

6. Titration
Titration of a strong acid with a strong base
ENDPOINT = POINT OF NEUTRALIZATION =
EQUIVALENCE POINT
At the end point for the titration of a strong acid
with a strong base, the moles of acid (H+) equals the
moles of base (OH-) to produce the neutral species
water (H2O). If the mole ratio in the balanced
chemical equation is 1:1 then the following
equation can be used.
MOLES OF ACID = MOLES OF BASE
nacid = nbase
Since M=n/V
MAVA = MBVB

7. Acid-Base Indicators
Finding the equivalence point of a titration
Use a pH meter
- Plot pH versus titrant volume
- Center vertical region = equivalence point
Use an Acid-Base Indicator
- Acid-Base Indicator = molecule that changes color based on pH
- Choose an indicator that changes color at the equivalence point
- End Point = when the indicator changes color. If you have chosen the
wrong indicator, the end point will be different than the eq. pt.
- Indicators are often Weak Acids that lose a proton (causing the color
change) when [OH-] reaches a certain concentration
HIn + OH- In- + H2O

9. Technique Of
Titration

10. TITRATION
MAVA = MBVB
Example:
1.Suppose 75.00 mL of hydrochloric acid was required to
neutralize 22.50 mLof 0.52 M NaOH. What is the
molarity of the acid?
HCl + NaOH  H2O + NaClMa Va = Mb Vb rearranges
to Ma = Mb Vb / Va
so Ma = (0.52 M) (22.50 mL) / (75.00 mL)
= 0.16 M
Now you try:
2. If 37.12 mL of 0.843 M HNO3 neutralized 40.50 mL of
KOH, what is the molarity of the base?
Mb = 0.773 mol/L