Conductometric Titration Essay

1513 Words4 Pages

It is highly beneficial to be able to calculate the concentration of a saturated solution. Indeed, knowledge of the concentration is required to calculate solute solubility and if precipitates will form when the solution is mixed with other reagents. This has many applications in industrial processes. For these reasons, this experiments aims to determine the concentration of a saturated barium hydroxide (Ba(OH)2) solution by conductometric titration and gravimetric analysis. Conductometric titration involve examining the change in Ba(OH)2 (aq) conductivity as sulphuric acid is added. Conductivity initially has a high reading due to the presence of ions in solution and then reaches a minimum at the reaction endpoint, due to complete neutralisation …show more content…

The mixture was then cooled. Vacuum filtration was then performed on the mixture. This was done by carefully rinsing the precipitate mixture over moist, pre-weighed filter paper into a Büchner flask under vacuum. The residue was then moistened with ethanol while the flask was still under vacuum. The residue and filter paper were placed on a pre-weighed watch glass and weighed. They were then placed in a drying oven for about fifteen minutes and then reweighed. They were reweighed after a further five minutes in the oven and then again after another five minutes, so as to ensure the precipitate had been fully dried. Results from both the conductometric titration and gravimetric analysis were compared with other groups and mean values were established. The experiment achieved its purpose in that the concentration of Ba(OH)2 solution was determined. According to the conductometric titration, the concentration of Ba(OH)2 (aq) was 0.196 M. Calculations based on gravimetric analysis revealed a concentration of 0.0669 M. Evidently, there is a high degree of imprecision between the values determined by each technique. It appears however that the gravimetric analysis was more accurate. The standard deviation for BaSO4 mass was 0.035 and …show more content…

According to the conductometric titration, the concentration of Ba(OH)2 (aq) was 0.196 M. Calculations based on gravimetric analysis revealed a concentration of 0.0669 M. Evidently, there is a high degree of imprecision between the values determined by each technique. It appears however that the gravimetric analysis was more accurate. The standard deviation for BaSO4 mass was 0.035 and the confidence interval was ±0.0256 g. This illustrates that there is 90% certainty that the actual mass of the BaSO4 precipitate was within 0.0256 g of the calculated mean (0.156 g). It should be noted that an outlier (1.45 g precipitate) was removed from the gravimetric analysis calculations due to being 9.29 times greater than the average. The standard deviation for end point volume – the basis of calculations for the conductometric titration – was 6.616. The confidence interval was ±5.443 mL. The much larger confidence interval for end point volume illustrates a higher degree of uncertainty regarding the precision of this measurement. For this reason, it appears that gravimetric analyses are more suitable for determining saturated solution concentration. This has importance in research where the solubility product (Ksp) needs to be determined or when predictions need to made regarding whether a precipitate will form. One of the principle reasons why conductometric titration

More about Conductometric Titration Essay

Open Document