Why did we have to use the same thermometer for finding, the freezing point of both, solvent and solution?
If your thermometer was not calibrated (reading 0.05 degrees Celsius below the correct temperature), how would this effect your measured value of delta Tf? Explain.
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Using the same thermometer for finding the freezing point of both the solvent and solution is important because it ensures consistency and eliminates any potential variation between different thermometers. This allows for more accurate and reliable measurements.
In scientific experiments, it is essential to control as many variables as possible in order to obtain accurate results. By using the same thermometer, any variations or biases introduced by different thermometers are eliminated. This helps to ensure that any observed differences in the freezing points are solely due to the presence of solute particles in the solution.
Now, if the thermometer used for measuring the freezing point was not accurately calibrated (reading 0.05 degrees Celsius below the correct temperature), it would affect the measured value of delta Tf (the freezing point depression). This is because the measured value of delta Tf is obtained by subtracting the freezing point of the solution from the freezing point of the pure solvent.
If the thermometer consistently reads 0.05 degrees Celsius lower than the actual temperature, it would cause the measured freezing point of both the solvent and the solution to be lower than their actual freezing points. Consequently, the calculated delta Tf would be smaller than the true value. This bias would affect the accuracy of the results and potentially lead to incorrect conclusions.
Therefore, it is crucial to ensure that the thermometer used for measuring the freezing point is properly calibrated to obtain accurate and reliable results.