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Acid-base Titration
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| Submitted: Fri Aug 15 2003
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S.6A Karen Kwok (8) 11th, September, 2002. Chemistry Laboratory Report Title: Acid-base Titration Date: 11th, September, 2002. Objective: (1) To determine the concentration of the unknown Sulphuric acid solution. (2) To learn how to use the pipette and burette skillfully. Result: The solution will change from yellow to orange when it is neutralized. 1st 2nd Final burette reading (cm3) 34.75 44.60 Initial burette reading (cm3) 9.55 19.25 Volume of sodium carbonate solution (cm3) 25.20 25.25 Calculation: The volumes of 0.0500M sodium carbonate required for neutralization are: 25.20 cm3, 25.25 cm3. Therefore the average volume of 0.0500 M sodium carbonate required for neutralization: = 25.20 + 25.25 2 cm3 =25.23 cm3 Na2CO3 (aq) + H2SO4 (aq) ›Na2SO4 (aq)+ CO2 (g)+H2O (l) 0.0500M ? M 25.00cm3 25.23cm3 No. of moles of sodium carbonate =Molarity of solution ×Volume of solution =0.0500 M ×0.0025 dm3 =0.000125mol According to the equation, 1 mole of Na2CO3 required 1 mole of H2S04 for complete neutralization. ?No of moles of H2SO4 = 0.000125mol Concentration of H2SO4 solution = No. of moles of...
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