required practicles

• How could you find out the volume of sulfuric acid that will exactly neutralise 25cm3 of sodium hydroxide solution?

  1. Place exactly 25cm3 of sodium hydroxide in a conical flask on a white tile, using a pipette and pipette filler

  2. Clamp the burette above the conical flask and fill it with sulfuric acid using a funnel, filling the burette to the 0.00cm3 line

  3. Add 5-10 drops of phenolphthalein to the conical flask

  4. Slowly add the sulfuric acid to the flask, swirling the flask at the same time

  5. Close the burette tap as soon as the mixture turns from pink to colourless

  6. Record the final volume of sulfuric acid added
• Apparatus required to carry out a titration

  • Burette
  • Conical flask
  • Pipette and pipette filler
  • Funnel
  • Clamp and stand
  • White tile
• Why should a white tile be used in a titration experiment?

  The white tile is placed under the reacting mixture, making the colour change easier to see
• Why might a volumetric pipette and pipette filler be used to measure 25cm3 rather than a measuring cylinder?

  A volumetric pipette will measure 25cm3 more accurately so it is usually used for titrations
• What is the purpose of repeating a titration?

  To allow a mean titre to be calculated, reducing the effect of random error
• What colour is phenolphthalein in acid and alkali?

  • Acid - colourless
  • Alkali - pink
• Why is the first trial in a titration often called a 'rough' trial?

  The first trial gives an approximate idea of where the end point is so then for further titres you can be more precise as you know approximately what volume will be required for neutralisation
• What safety precautions should be undertaken when carrying out a titration?

  • Wear eyewear and be aware of the dangers of the chemicals used, e.g. H2SO4 is corrosive, NaOH is an irritant
  • The burette should be filled below eye level so there's no risk of it spilling and splashing your face
  • Any broken glassware needs to be cleared immediately
• Why are burettes used for titrations?

  Burettes allow the solution to be added drop by drop in very small quantities
• Apart from phenolphthalein, what other indicator could be used in a titration? What is the colour change?

  • Methyl Orange: Red (acid) to yellow (alkali)
  • Litmus Blue: Red (acid) to blue (alkali)
• If you know the volume of acid required to neutralise an alkali, how could you calculate the concentration of the acid, given the alkali concentration and volume?

  1. Calculate the number of moles of the alkali using the known volume and concentration

  2. Use the chemical equation to work out the ratio of acid and alkali that react and hence work out how many mole of acid have reacted

  3. Divide the moles of acid by the volume used in neutralisation
• If you know the concentration of an acid in mol/dm3, how could you convert this to g/dm3?

  Multiply the concentration in mol/dm3 by the molar mass (Mr) of the acid to give the value in g/dm3
• How could you prepare a sample of pure, dry copper sulfate crystals from a sample of insoluble copper oxide?

  1. React sulfuric acid with excess copper oxide

  2. Filter to remove the excess copper oxide

  3. Heat the solution to start evaporation

  4. Turn off the heat and leave until all the water has evaporated

  5. Left with copper sulfate crystals
• Write the chemical equation for the reaction between CuO and H2SO4
• Safety precautions when preparing a pure dry salt from an insoluble compound

  • Bunsen burner should be turned off or put on the safety flame when not in use
  • Sulfuric acid is corrosive so wear eye protection
• Methods of separating mixtures

  • Filtration
  • Crystallisation
• How can you separate an insoluble product from a solution?

  1. Filter paper placed in a funnel over a conical flask

  2. Pour mixture through the funnel

  3. Insoluble product left on the filter paper
• How can you separate soluble solids from solutions?

  1. Place the mixture in an evaporating dish

  2. Slowly heat the solution

  3. The solvent evaporates and the solution becomes more concentrated so crystals will start to form

  4. Keep heating the evaporating dish until you have dry crystals
• How could you separate a soluble solid from a solution, if the solid decomposes when heated?

  1. Pour the solution into an evaporating dish and heat gently

  2. When the crystals start to form, remove the dish from the heat and leave to cool

  3. Once cold, filter the crystals out of the solution and leave them in a warm place to dry
• what is rough tritration

  carried out to find the approximate value of the end point but not used in calculations of mean