1. Ammonia Titration Laboratory Activity
The Problem:
Determine the molarity (M) and percent basicity (by mass) of ammonium hydroxide by acid/base
titration.
Information:
1. Ammonia in water forms NH4OH. prep table)
2. Do not titrate ammonia samples of more than
10.0 ml at a time.
3. The burette at your lab station contains 1.2 M HCl.
4. Do no more than three trials.

2. Requirements and Goals of this Activity:
1. Work with your lab partner to summarize the
procedure, which must be checked before you
begin.
2. Record all data in a table.
3. Show all work for the calculations.
4. Assignment counts as a checked lab activity
(vs formal lab)

3. Titration of Ammonium Hydroxide Solution
Procedure:
●Mass an empty 125 ml Erlenmeyer flask.
●Measure 10.0 ml of ammonia and add to flask.
●Mass the flask with ammonia.
●Add 2-3 drops of phenolphthalein. (turns pink)
●Titrate with 1.2 M HCL until pink color
disappears (i.e. turns clear).

4. MEF & NH4OH ____0.01__ g _________ g MEF _________ g _________ g
Trial Trial 2
MEF & NH4OH ____0.01__ g _________ g
MEF _________ g _________ g
MNH4OH _________ g _________ g
NH4OH (100 ml buret)
Vf ____0.1__ mL ________ mL
Vi _________ mL ________ mL
Actual V used _________ mL ________ mL
HCl (50 ml buret)
Vf ____0.01__ mL ________ mL

5. (.00750 L HCl) (1.2 mol / L) = .0090 moles HCl
Calculations:
  NH4OH + HCl  NH4Cl + H2O
( )
( L HCl) (1.2 mol / L) = moles HCl
(.0090 mol HCl )(1 mol NH4OH) = .0090mol NH4OH
(1 mol HCl)
.0090 moles NH4OH = 0.9 M NH4OH
.0100 L solution (0.81 – 0.99)
(.0090 moles NH4OH) (35.0 g ) = g NH4OH
(1 mol NH4OH) (0.29 – 0.35)
N = 14.0
5 H = 5.0
O = 16.0
35.0  0.32 g NH4OH x 100% = 3.2 %
9.98 g solution (2.9 – 3.5)
( )