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Acid base titration. Aim: To determine the molarity of an unknown concentration of sulfuric acid.

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Introduction

Acid ? base Titration Aim: To determine the molarity of an unknown concentration of sulfuric acid. Data Collection: Trail 1 Trail 2 Trail 3 Final burette reading(ml) 12.50 24.70 37.15 Initial burette reading(ml) 0.0 12.50 24.70 Volume of Base NaOH(ml) 12.50 12.20 12.45 Molarity of NaOH 0.50 0.50 0.50 Volume of Acid H2SO4 10.0 10.0 10.0 Data processing: 1) H2SO4 + 2 NaOH ------------------- Na2SO4 + 2 H2O According to the above equation : Ratio between moles NaOH : H2SO4 2 : 1 2) At the endpoint: 2(no. mole of acid) ...read more.

Middle

0.0 12.50 24.70 Volume of Base NaOH(ml) 12.50 12.20 12.45 Molarity of NaOH(base)M 0.50 0.50 0.50 Volume of Acid H2SO4 (ml) 10.0 10.0 10.0 Molarity of H2SO4 (acid) M 0.3125 0.305 0.31125 Average Molarity of H2SO4 (acid) M 0.309 XXXXXXX XXXXXXX 3) 0.3125M + 0.305M + 0.31125M = 0.309 M 4) According to the above equation : Ratio between moles NaOH : H2SO4 2 : 1 At the endpoint: 2(no. mole of acid) = no. of mole of base 2(Molarity of acid*Volume of acid) = Molarity of base*volume of base 5)KOH + HCl ------------------ KCl + H2O At the endpoint: no. ...read more.

Conclusion

This indicator was phenolphthalein and the color change is pink. Moles relationship has to be taken in consideration according to the theoretical equation. Accuracy has to be high in doing the experiment because it is a quantitative one. Such experiments are very helpful in understanding concentrations of solutions and measuring volumes and relating that to moles. Source of error: 1. Inaccurate measurements of volumes 2. Having impurities in the burette or flasks 3. Exceeding the endpoint , this can be known by the color of the indicator Improvements: 1. Controlling the addition of the drops of base using a more advanced way 2. Starting from zero always in each trail ...read more.

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