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

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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.

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