• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Find the exact concentration of sulphuric acid in a solution through a titration.

Extracts from this document...

Introduction

Salters Chemistry coursework Aim: To find the exact concentration of sulphuric acid in a solution through a titration. The titration is between sulphuric acid and sodium carbonate has to be in liquid for in order to carry out the experiment so it is dissolved into distilled water to a concentration of 0.1 mol dm� Introduction- During the extraction of a metal from its ore, sulphuric dioxide is often produced. This is converted to sulphuric acid and is sold as a useful by-product. I am going to be given a sample of sulphuric acid, which is thought to have a concentration between 0.05 and 0.15-mol dm�. The purpose of this experiment is to find the accurate concentration of the sulphuric acid. I will do this by carrying out a titration between sulphuric acid and sodium carbonate solution. Therefore this is an acid-alkali titration (which is the determination of concentration by adding measured amounts of standard reagents to a known volume until the end point is reached). * Sulphuric acid is considered a strong acid, as it is completely in the form of ions in dilute solution. * Sodium carbonate is a weak alkali as it only partially forms ions in dilute solution. ...read more.

Middle

Keep the flow rapid till the colour changes to a lighter red, but before this turn the stopcock slightly horizontal as the acid comes out drop by drop. 12. Read off the value on the burette find out the volume of sulphuric acid needed to react with sodium carbonate. 13. Carry out the titrations Until you have recorded three results within 0.1cm� CONTROL VARIABLES Ensure the same sodium carbonate solution and sulphuric acid batch is used for all titration to ensure a fair test and the results will be accurate and reliable. Try to carry out the titrations on the same day to ensure there isn't a temperature change and that they are done in one uniform temperature. If the temperature is increased, the liquid will expand making the test inaccurate. RISK ASSESMENT * Wear safety goggles to prevent acid from entering the eye * Stools must be tucked underneath the table ensure bags are out of the way to prevent people from tripping * Long hair should be tied back * Ensure you are standing throughout the experiment so you are able to quickly move out of the way in case of spillages etc. ...read more.

Conclusion

It was important to keep a specific colour in mind, and stop the titration when the colour was reached. Fortunately I kept the colour change point constant, although this could have been a cause of any anomalies. To improve the investigation a pH metre can be used instead of using a pH indicator to see when neutralisation occurs. This would eliminate the most significant source of error, which is largely due to human error. I could have further improved the experiment by checking the pipette filler for air gaps. Also using a magnetic stirrer would have ensured all the sodium carbonate was completely dissolved. I could have used more accurate scale -analytical balance which measure to 0.0001g so it has a high degree of precision Percentage error I am going to work out the percentage error using the following equation: (True value- experimental value) � 100 True value Quantity measured Percentage error Mass of sodium carbonate using balance (0.05�100)/2.65=0.19% Volume of distilled water using volumetric flask (0.5�100)/250=0.2% Transferring sodium carbonate using pipette filler (0.5�100)/25=2% Carrying out titration using a burette (0.005�100)/28.43=0.02% (to 2.s.f) In order to minimise measurements errors larger quantities of all solution could be used although concentration would remain the same. For example 250 cm� graduated flask 0.2 � 100 = 0.08% 250 1 dm� flask 0.2 �100 = 0.02% 1000 Saher Ali 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. Marked by a teacher

    Enthalpy of Neutralisation.

    3 star(s)

    This leads me to think that if 2M of alkali were reacted with 1M of acid only half the ions are reacted to form the neutralisation reaction so less energy is produced.

  2. In this experiment, we aim to investigate the effect of sodium carbonate on hard ...

    So the sodium carbonate effectively lessens the effect of calcium ions in the water, thus softening it and making it easier for a lather to be formed. The calcium carbonate is precipitated and this removes the hardness from the water.

  1. In order to find out the exact concentration of sulphuric acid, I will have ...

    However once there is an excess of acid present, the curve should gradually even out. Furthermore at the very beginning of the curve, pH will decrease quite rapidly once the acid is added, but soon after that the gradient should decrease.

  2. Determine the concentration of sulphuric acid by acid-base titration.

    * White paper: used to place behind the burette to obtain a clear reading. * Goggles: used for eye protection through out the experiment. Chemical hazard notes: A hazard is anything that can cause harm if things go wrong. Hazards include: - Chemicals (such as corrosive acids and alkalis, toxic gases and chemical which cause cancer)

  1. Finding out how much acid there is in a solution.

    Sub substance Formula Mass of 1 mole (in grams) Sulphuric Acid H2SO4 (2 x 1) + (1 x 32) + (4 x 16) = 98 Sodium carbonate Na2CO3 (2 x 23) + 12 + (3 x 16) = 106 (a)

  2. Titration I will neutralize the sulphuric acid with a base, which will be Sodium ...

    I must calculate the mass of Sodium Carbonate used in the solution... Mass used 2.65 grams = =0.025 mols in 250ml Mass of Sodium Carbonate 106 grams To convert this to 1 litre I must multiply by 4 0.025 X 4 = 0.1 mols in a litre I will use

  1. How much Iron (II) in 100 grams of Spinach Oleracea?

    0.0000525 mol dm-3 x 5 = 0.0000875 mol dm-3 3 Now that I know the mols of Iron (II) present in 5 cm3 of spinach extract solution I can use this to work out the moles of Iron (II) present in 100 cm3 of spinach extract solution.

  2. Titration - The purpose of our experiment is to find the concentration of a ...

    Then pour the rest of the distilled water. 4. Stir with glass rod so that the solid is fully dissolved. 5. You should be left with 250cm3 of 0.1 mole dm3 sodium carbonate solution. Method of Titration 1. Attach clamp to stand and then clamp the burette vertically (place the

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work