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 inaccuracy between the values ​​determined by each technique. However, it appears that the gravimetric analysis was more accurate. The standard deviation for the mass of BaSO4 was 0.035 and the confidence interval was ±0.0256 g. This shows that there is a 90% certainty that the actual mass of the BaSO4 precipitate was within 0.0256 g of the calculated average (0.156 g). Of note, one outlier (1.45 g of precipitate) was eliminated from the gravimetric analysis calculations as it was 9.29 times greater than the average. The standard deviation for the endpoint volume – the basis of conductometric titration calculations – was 6.616. The confidence interval was ±5.443 ml. The much wider confidence interval for the end point volume illustrates a higher degree of uncertainty regarding the precision of this measurement. For this reason it seems that gravimetric analyzes are more suitable for determining the concentration of the saturated solution. This is important in research where the solubility product (Ksp) needs to be determined or when predictions about the formation of a precipitate need to be made. One of the main reasons why conductometric titration