A conductometric titration of a saturated Ba(OH)2 solution with 0.05 M H2SO4 was performed in the following manner. A rinsed 50 mL burette was filled with H2SO4 solution and placed above a beaker containing accurately measured 10.0 mL sample of Ba(OH)2 solution and 50 mL distilled water. It was ensured that bubbles were removed from the burette. The LabQuest conductivity probe was set to 1-20, 000 μS cm-1 and calibrated out of solution. Before the addition of H2SO4, the conductivity of the Ba(OH)2 solution was recorded on LabQuest. 1 mL H2SO4 was added to the beaker and stirred. The conductivity and cumulative volu...
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...bottle of Ba(OH)¬2 and used different volumes of acid to reach the endpoint, indicates that the Ba(OH)2 (s) that fell out of solution was influencing the concentration of Ba(OH)2 (aq) aliquots each group used in the titration. Some groups may have pipetted from the bottom of the Ba(OH)2 bottle and picked up some Ba(OH)2 (s). This would have reduced the concentration of their Ba(OH)2 (aq) aliquot. Thus, they would have required less acid to cause neutralisation. A similar amount of solid would have been weighed as groups who had no Ba(OH)¬2 (s) in their aliquot because any minimised precipitate formation would have been offset by there already being Ba(OH)2 (s) present in the aliquot. In future, a fresh saturated solution of Ba(OH)2 should be used each time a titration is performed so that less Ba(OH)2 (s) can fall out of solution and negatively impact results.
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