Volumetric Vinegar Analysis
Experiment 9 and 10: Volumetric/Vinegar Analysis
Abstract:
The goal of the experiment that was conducted was to figure out both the molar concentration of NaOH and the standard mole ratio of the NaOH solution. In order to find the concentration of the NaOH solution, volumetric analysis was used. In volumetric analysis, a titration mechanism was utilized in order to find the reaction that the base will end up having with KHC8H4O4., also known as KHP. Phenolphthalein, which is the indicator that was used in this experiment, assisted in figuring out at exactly what point was there neutralization. The indicator turns the solution into a bright pink color once neutralization has occurred. In experiment 10, the average molarity of NaOH that was found in experiment nine was used in order to find out if the vinegar that was being used in the experiment contained around the same percent mass of acetic acid that is found in regular vinegar. The experimental value of NaOH that was used was 1.0425 grams and the molarity of NaOH was found to be 0.089 m/L of NaOH. Towards the conclusion of the experiment, the average percent mass of acetic acid was calculated and found to be 1.695%. Regular house hold vinegar’s average percent mass of acetic acid usually ranges to 4-5%. Based on the percent mass of acetic acid obtained in the experiment, the vinegar that was used in experiment 10 was clearly not house hold vinegar. The hypothesis for this experiment was, if the average percent mass of acetic acid ranged between 4-5%, then it is house hold vinegar. However, due to the results from the experiments conducted, this hypothesis was rejected.
In order to obtain the results that the groups were searching for, titration was used in both experiments to find the answer. The method of titration involves the measurement of KHP and NaOH. Afterwards, the volumetric analysis was used, with the indicator included. The
Abstract:
The goal of the experiment that was conducted was to figure out both the molar concentration of NaOH and the standard mole ratio of the NaOH solution. In order to find the concentration of the NaOH solution, volumetric analysis was used. In volumetric analysis, a titration mechanism was utilized in order to find the reaction that the base will end up having with KHC8H4O4., also known as KHP. Phenolphthalein, which is the indicator that was used in this experiment, assisted in figuring out at exactly what point was there neutralization. The indicator turns the solution into a bright pink color once neutralization has occurred. In experiment 10, the average molarity of NaOH that was found in experiment nine was used in order to find out if the vinegar that was being used in the experiment contained around the same percent mass of acetic acid that is found in regular vinegar. The experimental value of NaOH that was used was 1.0425 grams and the molarity of NaOH was found to be 0.089 m/L of NaOH. Towards the conclusion of the experiment, the average percent mass of acetic acid was calculated and found to be 1.695%. Regular house hold vinegar’s average percent mass of acetic acid usually ranges to 4-5%. Based on the percent mass of acetic acid obtained in the experiment, the vinegar that was used in experiment 10 was clearly not house hold vinegar. The hypothesis for this experiment was, if the average percent mass of acetic acid ranged between 4-5%, then it is house hold vinegar. However, due to the results from the experiments conducted, this hypothesis was rejected.
In order to obtain the results that the groups were searching for, titration was used in both experiments to find the answer. The method of titration involves the measurement of KHP and NaOH. Afterwards, the volumetric analysis was used, with the indicator included. The
Cited: Beran, Jo A. Laboratory Manual for Principles of General Chemistry. Hoboken, NJ: Wiley, 2011. Print. Tro, Nivaldo J. Principles of Chemistry: A Molecular Approach. Upper Saddle River, NJ: Prentice Hall, 2010. Print.