If a 3.90 m solution boils at 103.45 °C, what is the actual value of the van't Hoff factor, i, given that the boiling point of pure water is 100.00 °C and the ebullioscopic constant (Kb) is 0.512 °C/m?

A solution of a nonvolatile solute in water has a boiling point of 380.5 K. Calculate the vapor pressure of water above this solution at 338 K. The vapor pressure of pure water at this temperature is 0.2467 atm. Which of the following is the vapor pressure of water above the solution?

A solution of water (Kb=0.512 °C/m) and glucose boils at 103.56 °C. What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00 °C.

Chloroform has a normal boiling point of 61.2°C and a boiling point elevation constant (Kb) of 3.63°C·kg/mol. You dissolve 1.08 moles of a compound (non-electrolyte) into 8 grams of chloroform. What is the boiling point of this solution?

If 29.5g of sodium phosphate (Na3PO4) is dissolved in 500.0g of water, what is the boiling point of this solution? Assume the boiling point elevation constant (Kb) for water is 0.512 °C/m and the molar mass of Na3PO4 is 163.94 g/mol.

Some people add salt to water, claiming that the salt raises the boiling point of the water, which makes the food cook faster. If 323 g of NaCl is added to a 2.54 L pot of water, what is the new boiling point of the solution?

What is the boiling point of a solution of 0.150 mole Al(NO3)3 in 0.500 kg of water, given that the ebullioscopic constant (Kb) is 0.512°C m⁻¹?

What is the boiling point of a solution that contains 50.0 g of FeBr3 in 200.0 g of water, given that the boiling point elevation constant (Kb) for water is 0.512 °C/m?

At an elevation of 1.45×10^4 ft, what is the approximate boiling point of water?