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Summary EXPERIMENT STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION
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EXPERIMENT of STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION
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EXPERIMENT 12 A: STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTIONOBJECTIVE:
Sodium hydroxide solution of about 0.2 M is prepared in order to be used in Exp 12B. The
solution is then standardized, that is, its concentration is accurately determined, by titrating it
against a weighed sample of known acidic salt, potassium acid phthalate.
INTRODUCTION:
Sodium hydroxide is deliquescent (absorbs moisture from the atmosphere) solid. It cannot be
weighed accurately. Therefore, it is not possible to prepare a standard solution of sodium
hydroxide of accurately known concentration by weighing NaOH. A sodium hydroxide solution of
approximate concentration (0.2 M) is to be prepared. It is then standardized by titrating it against
an accurately weighed sample of potassium acid phthalate (KHP), HOOC-C6H4-COOK , which is a
primary standard acidic substance. A primary standard substance can be weighed accurately
because it is stable (does not decompose) and not hygroscopic (does not absorb moisture from the
atmosphere). The reaction between NaOH and KHP (molar mass 204.23 g/mole) is as follows:
NaOH + HOOC-C6H4-COOK Æ NaOOC-C6H4-COOK + H2O
By measuring the volume of the ~0.2M NaOH solution dispensed from the buret that is necessary
to react completely with a weighed sample of KHP, the exact concentration of NaOH solution is
calculated.
PROCEDURE:
Check out a buret from the stockroom.
A. PREPARATION OF THREE SAMPLES OF KHP
1) Clean three 125 ml Erlenmeyer flasks and rinse with distilled water. Label the
Erlenmeyer flasks as 1, 2, and 3 using a pencil.
2) Accurately weigh out by difference three samples of KHP into the three labeled flasks.
Each sample should weigh between 0.3g and 0.4 g.
B. PREPARING SODIUM HYDROXIDE SOLUTION OF APPROXIMATE
CONCENTRATION
1. Clean your 250 ml Erlenmeyer flask and rinse it with distilled water.
2. Meaure between 8 and 8.5 ml of 6M NaOH using a clean, but not necessarily dry 10 ml
graduate cylinder. The 6M NaOH reagent bottle is on your bench.
3. Pour the NaOH solution into the 250 ml Erlenmeyer flask and then add distilled water
until the top of the solution is at the flask’s neck. Mix the solution well by pouring into a clean but
not necessarily dry 400 ml beaker and then pouring it back into the 250 ml Erlenmeyer flask. Do
this several times to make certain the solution is thoroughly mixed.
4. Label the 250 ml Erlenmeyer flask and stopper it with a #6.5 rubber stopper which you
will find on the Chem 111 reagent shelf. Do not allow the rubber stopper to come in contact with
the NaOH solution. Be sure to keep the solution stoppered when you are not using it (H2O reacts
with CO2 in the atmosphere forming H2CO3). Also, mix the solution well each time before you use
it.
NOTE: YOU WILL BE USING THIS SOLUTION IN BOTH, THIS EXPERIMENT AND EXP
12B. IF YOU WASTE THE SOLUTION YOU MAY RUN OUT BEFORE YOU HAVE
FINISHED EXP 12B.
, C. PREPARATION OF THE BURET
Check out a 25 ml buret from the stockroom.
1. Rinse the buret with tap water, then rinse it with distilled water. Make the final rinsing of the
buret with about 3 ml of the NaOH solution you just prepared and make certain that you drain it
through the stopcock.
2. Attach the buret with stopcock closed to a buret clamp mounted on a ring stand. Fill the buret
above the zero mark with the NaOH solution. Open the stopcock to allow the excess solution to
drain. This will aid in removing the air pocket from the tip of the stopcock. Make sure that the tip
of the buret is filled with solution and that there are no air bubbles.
D. STANDARDIZATION OF THE NaOH SOLUTION
1. At your bench add about 50 ml of distilled water to KHP sample #1. Add 2 drops of
phenolphthalein indicator. Swirl to dissolve the KHP completely.
2. On the report sheet, record the initial reading of the NaOH solution in the buret to the nearest
0.02 ml. Ask your instructor to check your reading and initial your report.
3. Place a white sheet of paper under Erlenmeyer flask #1 to facilitate the detection of the end point
when noting the color change of the indicator. Titrate KHP acid solution sample #1 by slowly
adding NaOH from the buret and constantly swirling the flask until you have reached the end point.
This is indicated by the appearance of a faint pink color of phenolphthalein that persists for 30
seconds or more after swirling the flask. Take the final buret reading to the nearest 0.02 ml and
record it on your report sheet.
4. Refill the buret. Repeat the titration for the remaining two KHP samples. Record your data on
your report sheet.
5. STOPPER AND SAVE YOUR NaOH SOLUTION FOR USE IN EXPERIMENT 12B !!!!!
E. CALCULATION
1. Calculate the molar concentration of the sodium hydroxide solution using your data for each run.
2. Calculate the average molar concentration of the sodium hydroxide solution. THIS IS THE
VALUE THAT YOU WILL USE IN EXPERIMENT 12B.
3. Calculate the precision of your experiment as standard deviation and as % deviation.
Note: If your percent deviation is greater than 2% you will need to carry out additional
titrations until you have a minimum of three values for the molar concentration of
NaOH that deviate by less than 2%.
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