Titration Of Sodium Hydroxide Solution

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Titration is a technique of slowly adding either an acid to a base or base to acid, until the equivalence point is reached. At the equivalence point, the number of moles of the titrant added corresponds to the number of moles of the substance being titrated. The titration technique is used to carry out a chemical reaction between two solutions by the controlled addition from a burette of one solution to the other, allowing measurements to be made throughout (Anne Marie, 2014). In order to observe the equivalence point, an indicator must be added to one of the solutions. The colour of the solution will change in colour depending on the type of indicator and the nature of solution. For example, Phenolphthalein is pink in a basic solution and …show more content…
Investigative question: How will the volume of Oxalic acid affect the concentration of the Sodium Hydroxide?
Hypothesis: A large volume of Oxalic acid will neutralise 20ml of Sodium Hydroxide.
Dependant Variable: Concentration of 20ml Sodium Hydroxide solution.
C_NaOH=n/V
Therefore, [NaOH] is directly proportional to it number of moles, and inversely proportional to its volume.
Independent Variable: Average volume of Oxalic Acid solution titrated against the 20ml Sodium Hydroxide solution.
Controlled Variables: The volume of Sodium Hydroxide solution; only 20ml of Sodium Hydroxide was neutralized in each of the three titration trials. Only De-ionized water was used to make the solutions and rinse the equipment. The temperature of the water and the solutions was neither increased nor decreased (temperatures were at room temperature).
Apparatus:
1 50ml burette 1 Electronic scale
1 Glass funnel 3 Erlenmeyer Flasks
2 250ml Volumetric Flasks 1 Suction …show more content…
Label the solution: Sodium Hydroxide

Prepare the titration

Place another clean funnel into the 100ml burette and pour the Oxalic acid solution through the funnel and into the burette. Make sure the bottom of the meniscus reaches the mark that reads: 0ml. Rinse the pipette with deionised water and use it to draw 10ml of sodium hydroxide solution. Release the solution into a clean Erlenmeyer flask, labelled “A”. Draw another 10ml of Sodium Hydroxide and release it into the same Erlenmeyer flask to make up 20ml of Sodium Hydroxide solution. Add 4 drops of Phenolphthalein indicator into the Sodium Hydroxide solution. The solution should change from colourless to dark pink, showing that Sodium Hydroxide is a base. Place the pink Erlenmeyer flask under a standing burette and on a white piece of paper. Open the Burette tap to release the oxalic acid solution and begin the acid-base titration. Swirl the pink Erlenmeyer flask after every 3 drops of oxalic acid to increase the rate of reaction. The colour should change from dark pink to light
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