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

Titration To Determine the Concentration of a Solution of Sulphuric Acid.

Extracts from this document...

Introduction

TITRATION TO DETERMINE THE CONCENTRATION OF A SOLUTION OF SULPHURIC ACID. Introduction The volume of unknown sulphuric acid needed to neutralize the sodium hydroxide using bromothymol blue. You simply titrate the unknown sulphuric acid against the solution of sodium hydroxide with a known concentration. Then when you have calculated the concentration of the acid you can use it in turn as a standard solution, to find the concentration of the solution of alkali. (Acids are substances which donate protons and the bases are substances which accept them) 2NaOH + H2SO4 --------- Na2SO4 + 2H2O Safety The sulphuric acid is corrosive. The sodium hydroxide is caustic. At all times through the experiment you must wear eye protection and lab coats. When filling the pipette be careful it does not break. ...read more.

Middle

Calculate the volume of acid used. Carry out four titrations, one trial and three accurate. Give your answer to 2 decimal places. Results Titrations Initial reading Final reading volume used cm3 1 0.00 27.55 27.55 2 0.55 27.10 26.55 3 0.00 26.50 26.50 4 0.00 26.40 26.40 Calculations Average volume of unknown sulphuric acid used, from three accurate titrations: 26.55 + 26.50 + 26.40 = 26.48 cm3 Moles of HaOH = Concentration * volume in dm3 = 0.2 * 0.025 = 0.005 moles From the equation 2NaOH + H2SO4 --------- Na2SO4 + 2H2O 1 mole of NaOH = 0.5 moles of Na2SO4 Concentration = moles / volume 0.005 moles of NaOH = 0.0025 moles of Na2SO4 Concentration of Na2SO4 = moles / volume = 0.0025/ 26.48/1000 = 0.0025/ 0.02648 = 0.094 moldm3 Conclusion The morality of the unknown sulphuric acid was 0.094 moldm3. ...read more.

Conclusion

The reading could not be exactly clear due human usage of the instrument time after time. Pr�cis accuracy. The numbers could have been blurred so you can not read it to. The meniscus of the solutions could be out a little. We could have lost some of the solution when we were transferring it from the pipette to the conical flask. It could have remained on the side of the pipette and the conical flask. We could not collect all the solutions no matter how hard we tried. Due to equipment error. Instrument accuracy/ lowest reading * 100 = ans 0.05/ 26.40 * 100 = 0.19 This shows that the equipment are not absolute accurate. Another factor could have been the air around us. Or standing near the window and the outside temperature could have its effect. Other instruments could be used which have a better accuracy point. More sophisticated measuring equipment could also be another point to notice. ...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 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)

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

    Pour further distilled water into the beaker until the beaker is filled half way(150cm3) 7) Used the glass rod to stir the solution until the solid has dissolved. 8) Transfer the solution into Graduated volumetric flask using a funnel so that all the solutions get into the flask. 9)

  1. Experiment to determine the concentration of sulphuric acid

    is used to wash the pipette . The sulphuric acid is used to wash the burette. 25 cm� of the aqueous solution of sodium hydroxide is put into a conical flask using a pipette and filler. The amount in the pipette is seen from the line on the pipette which shows 25 cm� of solution.

  2. To carry out a titration between a strong acid and a weak alkali, to ...

    Add the sulphuric acid solution from the burette to the conical flask by turning the stopcock on the burette vertical. Keep the flow of acid into the conical flask rapid, until the solution starts turning lilac at the centre, as it is more concentrated under the tap.

  1. Find the accurate concentration of a solution of sulphuric acid acid of which concentration ...

    3.98g and use it to make a solution of Na2CO3 of concentration between 0.05 and 0.15moldm-3 . PROCEDURE: 1. I will tranfer some quantity of solid anhydrous Na2CO3 into a mortar and grind it using a pestle till fine powder is obtained.

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

    solution in Burette and clamp To place sulphuric acid in and efficiently pour in to beaker Pipette and pipette filler Mentioned in method Funnel Volumetric Flask METHOD 1. Weigh mass of boat set scales to 0 then add 2.65g of anhydrous sodium carbonate to the boat using a spatula 2.

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