An acid-Base titration is a common practice in any laboratory setting. During analysis samples in the lab, for accurate and precise results is very important to use clean apparatus, calibrated equipment and standardized chemical reagents. In practical one during the standardization of NaOH, a standard solution of HCl is used to determine the correct concentration of the 1.0N NaOH prepared solution. From the reacting ratios between the acid and the base, the moles of the HCl is determined upon titrating the acid against the base. The moles of the acid is equivalent to the moles of the base due to 1:1 mole ratio. The concentration of the base is then calculated.
In part B, the molecular mass of unknown acid concentration can be calculated provided the attention of the base is known. It is also important to note that the weight of the unknown acid.
Should be provided. The validity of the results in part B very close since the acid consumed almost the amount of the base. During the experiments, there were some courses of error, for instance, reading the burret below the meniscus interfered with titer volumes affecting the final results. Also, during the preparation of NaOH solution, NaOH is hydroscopic compound hence to get exert weight during the weighing was a challenge. These also interfered with results.
During the experiment in part C, the average molar mass of the acid was determined by calculating it from the reacting potentials of 1:1 mole ratio. The average molar mass of the diprotic acid was close to the exert molar mass of the diprotic acid. The difference was an error encountered during the titration of the acid. The practical has a wide range of study, for instance, it is applied in gas laws, to determine volumes, pressure and concentrations of the reacting species.