Boiling-point elevation constants for

B. In the equation At = i m - Kb, where At is the boiling-point elevation, m is the molality of the solution, and Kb is the boiling-point-elevation constant for water, i (the van t Hoff factor) would be expected to be 4 if H3B03 were completely ionized. According to data provided, i is about 1.5. Therefore, H3B03 must have a relatively low Ka. 

What is the molality of an aqueous glucose solution if the boiling point of the solution at 1 atm pressure is 101.27°C The molal boiling-point-elevation constant for water is given in Table 11.4. 

A solution prepared by dissolving 5.00 g of aspirin, C9H8O4, in 215 g of chloroform has a normal boiling point that is elevated by AT = 0.47°C over that of pure chloroform. What is the value of the molal boiling-point-elevation constant for chloroform ... 

A solution of citric acid, C HsC, in 50.0 g of acetic acid has a boiling point elevation of AT = 1.76°C. What is the molality of the solution if the molal boiling-point-elevation constant for acetic acid is Kb = 3.07 (°Okg)/mol. 

Freezing Point Depression and Boiling Point Elevation Constants for Various Solvents... 

The boiling-point elevation constant for water is 0.512°C/m (see Table 15.3). Thus,... 

When 1.645 g of white phosphorus are dissolved in 75.5 g of CS2, the solution boils at 46.709°C, whereas pure CS2 boils at 46.300°C. The molal boiling-point elevation constant for CS2 is 2.34°C/m. Calculate the molar mass of white phosphorus and give the molecular formula. 

EXAMPLE 7 Calculate the value of the boiling-point-elevation constant for a solvent that boils at 53.8°C and for which a 0.359 m solution boils at 55.8°C. 

Calculate the boiling-point elevation constant for each of the following substances. 

Table 12.2 lists values of A), for several common solvents. Using the boiling-point elevation constant for water and Equation (12.6), you can see that if the molality of an aqueous solution is 1.00 m, the boiling point will be 100.52°C. 

Using Equations 9.21 and 9.24 and data from Tables 7.7 and 7.8, calculate the freezing-point depression and boiling-point elevation constants for diethyl ether. 

Use the data in Table 12.4 to evaluate the molal freezing-point depression constant and the molal boiling-point elevation constant for H2O at a pressure of 1 bar. 

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