Data Analysis
Table 1: Determination of the concentration of the Ba(OH)2 solution
| Parameter | Trial 1 | Trial 2 |
| Concentration of standardized H2SO4 solution (M) | 0.0200 | 0.0200 |
| Volume of Ba(OH)2 solution (mL) | 50.0 | 50.0 |
| Volume of H2SO4 to the reach the equivalence point (mL) | 10.944 | 10.573 |
| Concentration of Ba(OH)2 solution (M) | 0.00438 | 0.00423 |
Figure 1: Conductivity vs Volume
Calculations
Concentration of Ba(OH)2
Trial 1
Trial 2
Conclusion
The purpose of this lab was to determine the concentration of Ba(OH)2 using conductivity. The equivalence point was reached when the two electrolytes, Ba(OH)2 and H2SO4 are combined in a stoichiometric ratio. That is when all of the ions are removed and the conductivity is at its minimum. The conductivity increases if more of the second electrolyte is added after the solution reaches the equivalence point. No chemical reaction occurs after the equivalence point is reached but ions are added from the second electrolyte being added. In this lab, Ba(OH)2 solution was titrated with H2SO4 solution. When the equivalence both was reached the ions Ba2+, OH-, H3O+, and (SO4)2- were not present. Once the equivalence point was determined, then the concentration of the Ba(OH)2 solution could be calculated.
The concentration of Ba(OH)2 was found to be 0.00438 M in trial 1 and 0.00423 M in trial 2, which the averages out to be about 0.00431 M. The equivalence point for trial 1 was 10.944 mL of H2SO4 and for trial 2 it was 10.573 mL of H2SO4. This is slightly off for the equivalence point of H2SO4 and Ba(OH)2 because it should be around 15 mL. The Ba(OH)2 solution was made with barium nitrate so it had extra ions which influenced the conductivity. Some sources of error in this lab could have come from not measuring out the chemicals accurately, and not making sure all of the beakers and jars were cleaned out before using them.