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Titration of an Unknown Potassium Halide Against Silver Nitrate

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Titration of an Unknown Potassium Halide Against Silver Nitrate Apparatus * 250cm3 volumetric flask + 0.3cm3 * 25cm3 pipette + 0.06cm3 * Filler * Conical flask * 50cm3 burette + 0.05cm3 * Retort stand and burette holder Chemicals * 1.035g + 0.001g unknown potassium halide * Distilled water * 0.1moldm-3 Potassium chromate indicator * 0.05moldm-3 Silver Nitrate Solution Data Collection Mass of solid white Unknown potassium Halide used: 1.035g +0.001g. This was made up to a 250cm3 colourless solution. 0.1moldm-3 yellow potassium chromate indicator was used in this titration. The end point was judged to be when a dark pink precipitate started to form. Rough Titration Titration 1 Titration 2 Titration 3 Initial Burette Reading + 0.05cm3 0.00cm3 18.80cm3 1.00cm3 18.40cm3 Final Burette Reading + 0.05cm3 18.80cm3 36.30cm3 18.40cm3 35.60cm3 Titre +0.1cm3 18.80cm3 17.50cm3 17.40cm3 17.20cm3 The average Titre = 17.50 + 17.40 + 17.20 = 17.36666...cm3 3 = 17.40 (4sf) ...read more.


Therefore 1 mole of KX = 1.035 . 8.70 x 10-3 = 118.9gmol-1 One mole of KX has an atomic mass of 118.9gmol-1. Atomic mass of one mole of KX = 118.9gmol-1 Atomic Mass of one mole of K = 39.10gmol-1 Therefore the atomic mass of one mole of X = 118.9 - 39.10 Atomic mass of X = 79.80gmol-1 Therefore X = Br The unknown potassium halide was Potassium Bromide. Percentage Uncertainty Percentage Uncertainty of Volumetric Flask = 0.3 . x 100 = 0.12% 250.0 Percentage Uncertainty of Pipette: 0.06 x 100 = 0.24% 25.0 Percentage Uncertainty of balance: 0.001 x 100 = 0.10% 1.035 Percentage Uncertainty of Burette: 0.1 x 100 = 0.57% 17.4 Overall Percentage Uncertainty of Equipment = 0.24 + 0.10 + 0.57 + 0.12 = 1.03% Effect of the total percentage uncertainty on the result [Atomic Mass KX = 118.9gmol-1] = 118.9 x 1.03 100 = 1.22gmol-1 (3sf) ...read more.


This may have resulted in the end point being overstepped, or not quite reached, which would have affected the accuracy of the results. Although there was a total percentage error on the equipment of 1.03%, this is negligible, as the greatest error on the results in this titration would be caused by personal judgement, as when the end point is judged to have occurred is dependent on the person carrying out the titration. The accuracy of the results obtained from this titration may be improved if the silver nitrate solution was held in a container that blocked out light. As a result of this, the silver nitrate would be less affected by the light, and consequently the end points of each titration would be more consistent, therefore improving the accuracy of the results. ?? ?? ?? ?? Emma Wellham 0502966 Titration of an Unknown Potassium Halide Against Silver Nitrate Page 1 of 3 ...read more.

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