The formula that governs the depression of freezing point and elevation of boiling point for a...

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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queen_honey_blossom answered 1 year ago

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