The molal elevation constant of water is 0.512C/m,therefore boiling point of 0.1m CaCl2 solution in water is expected to be
Addition of a solute increases the boiling point of solvent. which is given by the formula,
ΔTb = i Kbm
where, i = Van't Hoff factor
ΔTb = the amount by which the boiling point is raised
m = molality (moles solute particles per kg of solution)
Kb = molal boiling-point elevation constant (solvent dependent)
Since, CaCl2 is an electrolyte, so its Van't Hoff factor will be 3 ( CaCl2 ⇋ Ca2+ + 2Cl- )
Therefore, ΔTb = 3 0.512 oC m-1 0.1 m
= 0.1536 oC
Hence the new boiling point of water will be 100 oC + 0.1536 oC = 100.1536 oC
ΔTb = i Kbm
where, i = Van't Hoff factor
ΔTb = the amount by which the boiling point is raised
m = molality (moles solute particles per kg of solution)
Kb = molal boiling-point elevation constant (solvent dependent)
Since, CaCl2 is an electrolyte, so its Van't Hoff factor will be 3 ( CaCl2 ⇋ Ca2+ + 2Cl- )
Therefore, ΔTb = 3 0.512 oC m-1 0.1 m
= 0.1536 oC
Hence the new boiling point of water will be 100 oC + 0.1536 oC = 100.1536 oC