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13 Dec 2019

If the freezing point of the solution is erroneously read 0.2 degrees celcus lower than it should be, will the calculated molar mass of the solute be too high or too low?

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Irving HeathcoteLv2

17 Dec 2019

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If the freezing point of the cyclohexane solution is recorded 0.2 degrees Celsius lower than its actual freezing point, will the molar mass of the unknown be reported too high or too low? Explain.

yellowcaribou517

1) Some of the cyclohexane solvent vaporized during the temperature versus time measurement. Will this loss of cyclohexane result in its freezing point being recorded as too high, too low, or unaffected? Explain.2) The solute dissociates slightly in the solvent. How will the slight dissociation affect the reported molar mass of the solute - to high, too low, or unaffected? Explain. 3) Interpretation of the data plots consistently shows that the freezing points of three solutions are too high. As a result of this "misreading of the data," will the reported molar mass of the solute be too high, too low, or unaffected? Explain

erinmarten35

A student failed to clean their equipment resulting in an impurity during this experiment. The impurity is insoluble in water and was on the scoopula and therefore not in the test tube when it was tared. How will this reading affect the molar mass determination?

A) Too low. The impurity will cause the change in temperature to be larger, causing the mol solute to be too large. Since molar mass is g/mol, the molar mass will be calculated too low.

B) No affect. The impurity will cause the change in temperature to be larger, causing the mol solute to be too large. However, the grams of the solute will also be too large. Since molar mass is g/mol, the molar mass will not be affected.

C) Too high. The grams of impurity will be added to the mass of the solute. It will not cause a change in temperature since it is insoluble. Since molar mass is g/mol, the molar mass will be calculated too low.

D) No affect. The solute is insoluble and will not change the freezing point so the mol solute are unaffected. The grams of solute is also unaffected so molar mass will not be affected.

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If the freezing point of the solution is erroneously read 0.2 degrees celcus lower than it should be, will the calculated molar mass of the solute be too high or too low?

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