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Acid Base Titration Lab Report. The purpose of this experiment is to determine the concentration of a solution of Sodium hydroxide by titration against a standard solution of Potassium hydrogenphtalate.

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An Acid - Base Titration Aim: The purpose of this experiment is to determine the concentration of a solution of Sodium hydroxide by titration against a standard solution of Potassium hydrogenphtalate. The Importance of phenolphthalein in this experiment: the phenolphthalein indicator is important in this experiment for the following reasons; 1. It enables us to know the exact volume of the base needed to completely neutralize the solution of the acid. 2. It shows when the neutralization has come to the end point by turning slightly pink in the acid. 3. one can know that the neutralization has gone past the end point when the indicator turns darker pink Data Collection Qualitative data Color of acid before neutralization: Colorless liquid Color of acid close to the end point: Colorless with frequent pink color that disappears almost immediately as it is seen. Color of acid at the end point: slightest shade of pink that does not disappear within one minute. Temperature of room: 26.2�c Color of Base: Colorless solution. Color of phenolphthalein indicator before neutralization: Colorless liquid Color of phenolphthalein indicator after neutralization: slightly pinkish Quantitative data Table showing the number of trials performed in this experiment, the volume of the acid used, the volume of the base (NaOH) used, the number of phenolphthalein indicator drops used in each trial and the initial and final readings of the burette. ...read more.


Trials Volume of Sodium hydroxide(NaOH) /cm3 (�0.15%) Concentration of KHP/mol dm-3 Volume of Potassium hydrogen phthalate (KHP)/cm3 (�0.24%) Concentration of NaOH mol dm-3 (�0.39%) 1 26.55 0.10 25.00 0.1062 2 26.59 0.10 25.00 0.1064 4 26.54 0.10 25.00 0.1062 Average volume of KHP = 26.56 cm3 (�0.15%) Average Concentration of NaOH = 0.1062mol dm-3 (�0.39%) Conclusion The average concentration of NaOH derived from the calculations in this experiment is 0.1062 mol dm-3. The concentrations derived from each trial are very close to each other therefore the results could be valid. The major sort of error that affected my results was the calibrations on the burette - it was difficult to determine the volume of the NaOH. Since my results from the burette readings fall between 0.05 cm3, my results are therefore correct. Evaluation In this experiment, there were a number of errors that possibly occurred: 1. Leaving the funnel on the burette while titrating. Every drop in the experiment counts, by leaving the funnel on the burette, a drop or more of NaOH might get into the burette without one's knowledge can increase the volume of the base. In such a case as this, repeated trials while taking note of the position of the funnel will be the best way to reduce this error. ...read more.


Always make sure that the burette is full to at least 20.00cm3 before beginning titration. 6. Working at different areas of a room with slightly different temperatures. Difference in a room temperature could also cause results to be different. The higher the temperature difference in a room, the more likely it will be for results to be very different at different areas of the room. Check the temperature in the room before and during the experiment to ensure that there is little or no difference in the temperature around the room. 7. Titrating without any indicator. Without the indicator, there will be no color change in the conical flask containing the acid and the base. Ensure to add 2 or 4 drops of the indicator and swirl before beginning to titrate. Limitations and weaknesses 1. This experiment is restricted to an acid base neutralization. A precipitate cannot be used in this experiment. 2. The experiment cannot be stopped at the equivalence point as there are no materials to do that. It can only be stopped at the end point. 3. Leaving the funnel on the tip of the burette while titrating. This could increase the initial volume of the base making the result inaccurate. 4. Forgetting to refill the burette after each titration to avoid running out of the base in the middle of the titration. In this case, that particular trial will have to be done again. ?? ?? ?? ?? ...read more.

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