However, this temperature was lower than the boiling point of acetone, the most volatile solvent possibly present in the unknown solution, pointing to a source of error in the measurement of the temperature. This could have been due to an inaccurate thermometer or to an error in placing the thermometer too high. Because the boiling point was so low, the more volatile solvent was estimated to be acetone, which has a boiling point of 56.5°C. After fraction A was collected, the temperature of the stillpot was increased and should have produced a steady increase in a plot of the temperature versus total volume distilled while fraction B (a mixture of the two components) was collected, until a second plateau at the boiling point of the less volatile component. The temperature of the stillpot needed to be increased after collecting fraction A because the liquid left in the stillpot was then composed of a higher percentage of the less volatile component, with a correspondingly higher vapor pressure, meaning that it would boil at a higher temperature.…