Henderson Hasselbalch Titration Experiment

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Construction of titration curve for acetic acid, determining of the buffering capacity and influential factors
Abstract:
The experiment aims to measure the pH of solutions using the pH meter and by the Henderson Hasselbalch equation, which after comparison is made between the values. pH meter was used to measure the pH of the solutions and also the titration curve was established from the recordings of the pH and of volume of the base which was the NaOH. Factors that affect the buffer capacity were then evaluated and explained why they affect the buffer capacity. Calculations were done in results as determining the volumes and pH of the solution using the Henderson Hasselbalch equation. Further dilutions were done on some solutions determining factors that lead to the change in pH such as ionic strength. More factors were investigated referring to the published work in analytical chemistry. In conclusion, the buffer capacity is very sensitive and can be altered easily by adding either basic or acidic titrants.
Introduction:
The experiment looks at the behaviour of pH of the solution composed of weak acid and titrated by the strong base and the preparation of buffer in order to determine the buffering capacity of specific solution, moreover, it also looks at the factors affecting buffer capacity. pH is negative logarithmic of proton
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On the other volumetric flask, 0.2M of glacial acetic acid was prepared the acetic acid was anhydrous which does not contain water, it was poured to a volume of 100 ml and its density was 1.05 g/ml. Furthermore, the Henderson Hasselbalch equation was used to determine the volumes of each solution required to make a solution of 50 ml of 0.2M GIVEN THAT pH is 4.4 and pka is 4.76. Thereafter, appropriate volumes of each solutions were combined and pH was measured by the pH

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