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?

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.

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?

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 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?

What mass in grams of NaCl would need to be added to 2051 g of water to increase the boiling temperature of the solution by 1.500 °C? (Kb for water is 0.5100 °C/m)

What mass in grams of NaCl would need to be added to 2951 g of water to increase the boiling temperature of the solution by 1.500°C? (Kb for water is 0.5100°C/m)