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To determine the concentration of a solution of ethandioic acid.

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TO DETERMINE THE CONCENTRATION OF A SOULTION OF ETHANDIOIC [OXALIC] ACID INTRODUCTION In this experiment, the concentration of a solution of ethandioic acid will be determined by following two main steps, which include: Dilution of the Sodium Hydroxide. Titration of dilute sodium hydroxide and ethandioic acid. The indicator used will be phenolphthalein, which, will change from pink to colourless on neutralisation. Precautions Safety spectacles should be worn as acid is being used. Sodium hydroxide is caustic so care should be taken at all times. A white tile or white paper should be used to read off results to avoid errors. Any recordings should be taken at eye level and at the bottom of the meniscus. Dilution of Sodium Hydroxide (1.00mol dm-3) Apparatus and chemicals needed for the dilution; - 250ml volumetric flask - Dropper - Burette - Clamp and stand - Distilled water - 1 mol dm-3 NaOH solution - White tile or paper Procedure: 1. ...read more.


5. Stopper the flask and shake well [about 20 times] and label this solution A Titration of Sodium Hydroxide and Oxalic Acid Equation: [Ref.3] H2C2O4 (aq) + 2NaOH (aq) Na2C2O4 (aq) + 2H2O (L) Apparatus and chemicals needed: - 100cm3Burette - 25 ml Pipette - Phenolphthalein indicator; This organic compound (C20H14O4) used as an acid-base indicator. The compound is colourless in acidic solution and pinkish in basic solution. It does not dissolve very well in water so it is usually prepared in an alcohol solution. [Ref - Clamp and stand - White Tile - Conical flask - Dilute Sodium hydroxide [Solution A] - Oxalic Acid; Formula H2C2O4 is a colourless, crystalline organic compound that melts at 189 on sublimation. It has two ionisable H atoms; so two moles of NaOH are required to consume one mole of the acid. [Ref. 1] Procedure: 1. Set up the burette so that the clamp on the stand holds it. ...read more.


On seeing the change of colour, stop the tap and read off the burette reading [Place a white tile behind the burette scale in order to get an accurate reading]. Record this in your table. This result doesn't have to be exact as it is only a rough. 6. Repeat using the same method as above for two more accurate titrations. You will have to be more accurate for these two titrations as they have to be the exact amount of oxalic acid to neutralise the dilute sodium hydroxide. On reaching a point about 1-2cm^3 from the rough reading, close the tap and start adding the oxalic acid drop by drop so that the end-point can be determined accurately. The colour of the solution should change to completely colourless on the addition of one single drop. Record your results in the table below. Cross out the word 'Rough' if you regard that titration to be accurate. ...read more.

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