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

    1.33g Assuming the concentration of H2SO4 to be 0.15 moldm-3 , the concentation of Na2CO3 can be calculate as follows: Conc of H2SO4 (c) = 0.15 moldm-3 Volume of H2SO4 (v) = 25cm3 = 0.025dm3 Number of mole (n) = cv = 0.15 x 0.025 = 0.00375mols 0.025dm3 of Na2CO3

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

    During a successful collision they will interact, causing possible formation of covalent bonds and production of water molecules. There is very little tendency for this particular type of molecule to dissociate into ions again, which means that the concentration of H+(aq)

  1. Experiment to determine the concentration of sulphuric acid

    For accuracy, the amount should be looked from under the line. The hydrochloric acid is put into the burette using the funnel. It is measured to approximately 0.00 cm� but does not have to be exactly this. The number is recorded.

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

    This is why only one mole of sodium carbonate solution is needed to neutralise one mole of sulphuric acid. My first titration is an anomalous result because it did not require as much sulphuric acid to neutralise the sodium carbonate as the rest of my titrations did.

  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. How to find the accurate concentration of the Sulphuric Acid.

    Continue this until medical help can be obtained. -Ingestion will cause severe corrosion of and damage to the gastro-intestinal tract. In this case, do not induce vomiting, wash out mouth and drink water or milk. Seek medical attention immediately. -Inhalation could in the most severe case, cause pulmonary edema.

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