Neutralization of Naoh

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Neutralization Osaji Obi 3/28/2013 Introduction The objective of this experiment is to determine the neutralization curves for weak monoprotic and polyprotic acids, and to learn potentiometric pH measurement. Pka is also needed to be determined by the equation of –log(Ka). To find that we use half neutralization and titration with a strong acid. Procedure The solution is diluted to the mark with distilled water. A burette with the standardized NaOH solution is filled. The strength is recorded of the solution which it is marked on the dispensing bottle. Volume of the standardized base to neutralize the HOAc in the beaker is calculated. The electrodes are used to calibrate. The buffer is removed and rinsed with the electrodes with distilled water. It is then dipped in acetic acid and the pH is recorded. A burette was set up to add the NaOH. 1mL of NaOH is added. The solution is swirled and the pH is measured. The operation is repeated until equivalence point is met based on the above calculation. The base is added in increments. The increments are decreased when the pH begins to rise. Data See Graphs Calculations The calculations consisted of the deviations to create the pH curve graph. The Ka was calculated by taking the –log of the amount of acetic acid added and squaring it then dividing it by the amount of solution added. The moles for the NaOH was calculated by taking .1 moles and dividing it by 1,000 mL and then multiplying it by the amount of NaOH added. For the Molarity, the mole-mole ratio is used to convert it. Conclusion The pH curve came out zig zagged. The H3PO4 graph had two curves which was expected and my HOAc graph had 2 ½ curves. Based off the data the pH/Ka was right. The solution turned yellow indicating an acid on the pH scale. The Ka (9.1x10^-5) and

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