Question

The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: ΔT = i × kb × m

where: ΔT = the temperature change between a pure solvent and its solution

i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions; i = 2 for an ionic solute such as KBr that breaks apart into two ions, K+ and Br−, and so on) kb = a constant related to the solvent m = molality of the solute (molality, m = moles of solute / kg of solvent)

Using the above equation, how many grams of salt (CaCl2) would need to be added to 1 L of water in order for the boiling point of the solution to reach 108.5 °C? Assume that the density of water is 1.0 g/mL and that CaCl2 completely dissociates into three ions − i.e., a Ca2+ ion and two Cl− ions. The boiling point constant, kb, for water is 0.515 °C/m. Report your answer to the nearest 0.1 g

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Answer 1

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