Glucose freezing-point depression

The freezing-point depression of a solution relative to that of a pure solvent depends on the concentration of solute particles, just as boiling-point elevation does. For example, a 1.00 m solution of glucose in water freezes at — 1.86°C, and a 1.00 m solution of NaCl in water freezes at —3.72°C. The change in freezing point ATf for a solution is... 

You used 0.5 M glucose and 3% NaCl aqueous solutions in your tonicity experiments. What would be the freezing points of each of these solutions, considering that the freezing point depression constant of water is 1.86°C/osmol ... 

As we have seen, the colligative properties of solutions depend on the total concentration of solute particles. For example, a 0.10 m glucose solution shows a freezing-point depression of 0.186°C ... 

Using Numbers Calculate the boiling point elevation and freezing point depression of a solution containing 50.0 g of glucose (C6H12O6) dissolved in 500.0 g of water. 

Kb is the boiling point elevation constant, and for water equals 0.52°C/m. Each solvent has its own unique value for Kb, and the value of Kb for water indicates that a 1.0 m solution of glucose, a nonelectrolyte, would boil 0.52°C higher than that of pure water, 100.52°C. As with the equation used to calculate freezing point depressions, if the solute is an electrolyte, the molality of the ions will be a whole number multiple of the molality of the compound. 

Freezing-point depression is directly proportional to molality, so we first change the mole fraction of glucose to molality of glucose. Assuming that we have 1.0000 mol total, there are present 0.0555 mol of glucose and... 

Which of the following compounds would cause the greater freezing point depression, per mole, in H2O C6H12O6 (glucose) or NaCl ... 

B. Serum osmolality and osmolar gap. Serum osmolality may be measured in the laboratory with the freezing-point-depression osmometer or the heat-of-vaporization osmometer. Under normal circumstances the measured semm osmolality is approximately 290 mOsm/L and can be calculated from the results of the sodium, glucose, and BUN tests. The difference between the calculated osmolality and the osmolality measured in the laboratory is the osmo-lal gap, more commonly referred to as the osmolar gap (Table 1-22). 

The boiling point of 0.2 m solution of glucose is 100 + 0.1 = 100.1°C Freezing-point Depression... 

A solution consists of 10.3 g of the nonelectrolyte glucose, CgHj20g, dissolved in 250. g of water. What is the freezing-point depression of the solution ... 

It follows that 1 mol of sodium chloride will decrease the vapor pressure, increase the boiling point, or depress the freezing point of IL of water twice as much as 1 mol of glucose in the same quantity of water. 

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