Describe the experimental procedure to carry out a titration to find the exact volume of sulfuric acid needed to neutralise 25.0 cm3 of sodium hydroxide solution and obtain pure, dry crystals of sodium sulfate – 9044

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1. Titration and Preparation of Sodium Sulfate Crystals
   Rinse the pipette with sodium hydroxide solution and the burette with sulfuric acid to avoid contamination.

   Use a pipette to measure 25.0 cm³ of sodium hydroxide and transfer it into a conical flask placed on a white tile.

   Add a few drops of a suitable indicator such as phenolphthalein or methyl orange to the flask.

   Fill the burette with sulfuric acid and note the initial volume.

   Slowly add acid from the burette to the alkali while gently swirling the flask.

   Stop when the indicator changes colour, showing that the solution is neutral.

   Record the final volume of acid in the burette and calculate how much was used.

   Repeat the titration until you get concordant results (volumes within 0.1 cm³ of each other).

   Once you know the exact volume of sulfuric acid needed, repeat the titration without the indicator using the same volumes.

   Pour the neutral solution into an evaporating basin and heat gently or leave it to evaporate slowly.

   When crystals start to form, stop heating and leave the solution to cool.

   Filter the crystals, then dry them using absorbent paper.

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