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. Clearly, there is a high degree of inaccuracy between the values ​​determined by each technique. However, it seems that gravimetric analysis is more precise. The standard deviation for the mass of BaSO4 was 0.035 and the confidence interval was ±0.0256 g. This shows 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 one outlier (1.45 g of precipitate) was removed from the gravimetric analysis calculations because it was 9.29 times greater than the average. The standard deviation for the final volume – the basis of calculation for conductometric titration – was 6.616. The confidence interval was ±5.443 mL. The much larger confidence interval for the final 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 a saturated solution. This is important in research where the solubility product (Ksp) must be determined or where predictions must be made as to the formation of a precipitate. One of the main reasons why conductometric titration