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

The aim is to find the accurate concentration of sulphuric acid H2SO4 using titration with anhydrous sodium carbonate Na2CO3

Extracts from this document...

Introduction

Titration AIM: The aim is to find the accurate concentration of sulphuric acid H2SO4 using titration with anhydrous sodium carbonate Na2CO3 The following equation shows reaction (neutralisation) between sulphuric (VI) acid and sodium carbonate solution: Na2CO3 (aq) + H2SO4 (aq) Na2SO4 (aq) + CO2 (g) + H2O (l) This equation shows that one mole of sodium carbonate reacts with one mole of sulphuric (VI) acid. Therefore, they will always have the same number of moles when reacting with each other. We must follow the following steps to find the concentration of sulphuric acid: * We need to find the number of moles of sodium carbonate. We use the following formula to find the number of moles: Number of moles = the mass in gram/the molar mass = the mass/(23 X 2) ...read more.

Middle

2 Transfer the weighed sodium carbonate to a beaker and add 25 cm of distilled water to dissolve it completely and mix them. 3 After dissolving, transfer the solution to a 250 cm volumetric flask. Rinse the beaker thoroughly and transfer all the washes to the volumetric flask. Remember not to overshoot the graduation mark of the glass. 4 Make up the solution to the line on the neck by adding water. 5 Pipette 10 cm of sodium carbonate to a clean conical flask. 6 Add two drops of methyl orange indicator. 7 Fill up a 50 cm burette with sulphuric acid solution and add acid to the sodium carbonate in small volumes and swirl the flask after each addition. 8 Keep adding until you see the colour of sodium carbonate changes permanently. ...read more.

Conclusion

* The burette and the pipette should be washed out with the solutions being used. * The apparatus should be clean. * The end point of a titration can only be determined accurately if the acid from the burette is added drop by drop, with swirling, as the end point is reached. Risk assessment: * Lab coats should be worn during the experiment. * Eye protection should be worn. * Sulphuric acid causes severe burns. Solution equal to stronger than 1.5 M are corrosive. Solution equal to or stronger than 0.5 M but less than 1.5 M are irritant. If splashed in eyes, flood the eye with gently running tap water for 10 minutes. Seek medical attention. * Technicians must be informed if any spillage or breakage occur. * Hands must be washed after the experiment. Hassan Elumairi ...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. In this experiment, we aim to investigate the effect of sodium carbonate on hard ...

    So it has been proved that as one gradually increases the quantity of sodium carbonate used, the amount of soap solution needed to produce a lather also gradually decreases, until the plateau is reached. 4. EVALUATING Evaluation Overall, the experiment was a success in that it showed what it was

  2. Determine the Enthalpy of Neutralisation for the following there Acids, H2SO4, HNO3 and H2SO4

    Apparatus * Polystyrene cup * Glass Rod * Thermometer * Measuring Cylinder * 1 moldm-3 of HNO3 * 0.5 moldm-3 of H2SO4 * 1 moldm-3 of HCl * 1 moldm-3 of NaOH * Stop clock * Pen Paper, graph paper * Ruler * Calculator Method The heat released during a neutralisation (when 1 mole of water is formed)

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

    If swallowed: give plenty of water. Seek medical attention If substance gets in eyes: remove contaminated clothing. Wash off skin with plenty of water. Soak contaminated clothing and rinse repeatedly. If spilt in laboratory: scoop up as much solid as possible.

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

    Firstly the acid solution should contain san excess amount of H+(aq). At some point these ions should disperse randomly through out the possible solution. If basic OH(aq) ions are added to the solution, they will travel through the solution, until they meet a H+(aq)

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

    Sulphuric acid: If over 1.5mols it will cause severe burning if comes into contact with skin and eyes. It is very corrosive. I am using 0.1mols of sulphuric acid, which is very weak, but it is still quite irritant, so I will need to take care whilst using it.

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

    Finish (cm3) Titrate (cm3) 9.45 11.55 2.10 11.55 13.90 2.35 13.90 15.95 2.05 15.95 18.15 2.20 18.20 20.45 2.25 Average Titre = 2.10 + 2.05 + 2.20 + 2.25 +2.35 5 = 2.19 cm3 Analysing Evidence and Drawing Conclusions Experiment One - How accurate is a Potassium Manganate titration in determining the concentration of an Iron (II)

  1. Produce two different metal salts (NaHSO4 and Na2SO4) through an application of specific stoichiometric ...

    Using the molarity equation again; V = n/C V = (2.002x10-2mol)/(1.0707mol.dm-3) V = 0.01870 dm3 ? 0.05 % V1(H2SO4) = 18.70 cm3 ? 0.05 % This is the volume of sulfuric acid required to induce the reaction in (I), producing NaHSO4, as it will result in the presence of an equivalent number of moles for each reactant.

  2. To find the accurate concentration of sulphuric acid, by making up a standard solution, ...

    It has atoms and ions on its surface. To transfer the full atom and the ions, leave the glass rod in beaker. This gives you an accurate transference. 8 Get a clean funnel and place it into the volumetric flask.

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