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Standardization of sodium hydroxide solution using oxalic acid.

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Introduction

Title : Standardization of sodium hydroxide solution using oxalic acid. Results : 1. Preparation of the dilute H2C2O4.2H2O. 1. Mass of pure H2C2O4.2H2O : 1.6253 + 0.0001g 2. Volume in the measuring cylinder : 2.0 + 0.1cm³ 3. Volume in the volumetric flask : 250 + 0.5cm³ 1. Preparation of the Na2OH solution. 1. Mass of pure NaOH : 1.323 + 0.0001g 2. Volume in the volumetric flask : 250 + 0.5 cm³ 3. ...read more.

Middle

+ 0.1cm³ 29.60 29.00 27.50 Qualitative data : The colour indicator (phenolphthalein) in the NaOH solution changes from pink to colourless. The oxalic acid used to counterbalance the NaOH solution did not change a lot from its theoretical volume which is + 27cm³. Data processing : Gross volume of H2C2O4.2H2O used with uncertainty : 29.60 + 29.00 + 27.50 = 28.7 cm³ + 0.1 cm³. 3 Uncertainty : | 28.7-29.6 | + | 28.7-29.0 | + | 28.7-27.5 | x 100 = 8.4 % 28.7 Gross volume of H2C2O4.2H2O used with percentage of uncertainty = 28.7 cm³ + 8.4% cm³. ...read more.

Conclusion

So the number of moles of H2C2O4.2H2O with uncertainty = 0.0129 + 7.937 x 10-7 mol. The concentration of H2C2O4.2H2O : = Number of moles Volume (dm³) = 0.0129 mol 0.25 dm³ = 0.0516 mol/dm³. Uncertainty : ( 0.00025 + 7.937 x 10-7 mol ) (0.0516) 1. 0.0129 mol = 5.47748 x 10-5 mol/dm³. So the concentration of H2C2O4.2H2O with uncertainty = 0.0516 + 5.47748 x 10-5 mol/dm³. The concentration of diluted NaOH used : MaVa = a MbVb b Mb = 2 (0.0516 mol/dm³)(0.0287dm³) (1)(0.025dm³) = 0.1185 M. Conclusion : The concentration of NaOH that was used during titration method is 0.1185 M. ...read more.

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