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Titration of Sodium Hydroxide with HCI (using an indicator) and titration using a pH metre
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Titration of Sodium Hydroxide with HCI (using an indicator) and titration using a pH metre
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TITRATION OF SODIUM HYDROXIDE WITH HCI(USING AN INDICATOR)
EQUIPMENT
5x Beaker 200 ml
Sodium hydroxide of unknown concentration
Pipette
Pi-pump
Volumetric flask
Conical flask
Burette
Clamp stand
AIM
The aim of the investigation is to determine the unknown concentration of a sample of
sodium hydroxide. What I'm attempting to figure out is how titration, colorimetry, and pH
probe all have distinct techniques for determining the concentration of an unknown solution,
and how calculations all have different methods for calculating the unknown solution.
Titrations are most commonly used to determine the concentration of an unknown
component in a solution (the analyte) by reacting it with a solution of another material (the
titrant). The analyte concentration may be determined using the known titrant concentration,
the volume of titrant supplied, and the stoichiometry of the reaction. Although acid-base
titrations are the most common, there are various types. The titrant (NaOH), which is
gradually added throughout the titration, is introduced to the unknown solution. As it is
introduced, the HCl has progressively reacted away. The equivalence point occurs when just
the proper quantity of titrant (NaOH) is introduced to react with all of the analyte (HCl).
MAKING A STANDARDISED SOLUTION
I calibrate the balance using 1.45g weights, setting it to the right mass. I used a 50cm3
burette, a 100cm3 conical flask, a 100cm3 beaker, a 25cm3 pipette, methyl orange, a pipette
filler, a stirring rod, a Burette stand and clamp, white tile, a 0.1M sodium hydroxide solution.
To prepare a standard solution, I had to first properly measure 2.5g of anhydrous sodium
carbonate on a clock glass with a balance.
The sodium carbonate is then gradually transferred, stirring constantly, to roughly 50 cm3 of
distilled water in a clean 250 cm3 beaker. To ensure that all of the sodium carbonates has
been removed, I will use a wash bottle to rinse the clock glass with distilled water and add
the rinse to the beaker. Continue to stir the liquid with a stirring stick until the sodium
carbonate has completely dissolved. Wash the solution on the stirring rod with distilled water
into the beaker using a wash bottle. Transfer the solution into the 250 cm3 volumetric flask
using a clean funnel. Rinse the beaker several times with distilled water, then add the rinses
to the solution in the flask. Rinse the funnel with distilled water.
, This is part evidence for P1 and P2 - calibration and making standard
solutions
METHOD
Calibrate the pipette that you will be used with distilled water to eliminate any
undesired ions or minerals.
Transfer 25cm3 of sodium hydroxide solution (unknown concentration) into a 250cm3
conical flask with extreme caution and a few drops of methyl orange indicator.
Fill the burette with the standardised hydrochloric acid solution after cleaning it with
distilled water (same standardised solution from the titration before).
Titrate the sodium hydroxide solution with hydrochloric acid until the endpoint
indicator changes colour.
Record all data accurately and precisely to establish the exact titre of hydrochloric
acid necessary to achieve the endpoint of the titration.
You will need to do this as many times as necessary until you get the utmost
accurate results.
RESULTS
Rough 1st 2nd 3rd Averages
Initial volume 0 0 0 0 0
Vol of Na2Co3 used 27.5 27.7 27.6 27.7 27.6
(rough is not included for calculating the average)
Finding the concentration of sodium hydroxide solution using indicator
To find the concentration of sodium hydroxide solution, an indicator is used which is called
methyl orange. This is used to change the pH level, so a slight yellow colour is shown that
would indicate a basic medium.
Results were very predictable as in every pupil group, there will always be a colour change.
The only thing that would be identified as an inaccurate result is if the colour is very coloured
pink. What is only meant to be seen is a very pale pinkish peach. As such in the diagram
below.
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