What is the boiling point for a 3 molal #"CaCl"_2# aqueous solution? #K_b = 0.512^@ "C/m"#.

1 Answer
Aug 9, 2017

As you should have seen in your book,

#DeltaT_b -= T_b - T_b^"*" = iK_bm#,

where:

  • #DeltaT_b# is the change in boiling point in #""^@ "C"#, from that of the pure solvent, #T_b^"*"#, to that of the solution, #T_b#.
  • #i# is the van't Hoff factor, i.e. the effective number of solute particles in solution.
  • #K_b = 0.512^@ "C/m"# is the boiling point elevation constant of water.
  • #m# is the molality of the solution... #"mol solute/kg solvent"#. What is the solvent?

Assuming #100%# dissociation...

#"CaCl"_2(aq) -> "Ca"^(2+)(aq) + 2"Cl"^(-)(aq)#

and #1 + 2 = 3 ~~ i#, so...

#color(blue)(T_b) = T_b^"*" + iK_bm#

#= 100^@ "C" + 3 cdot 0.512^@ "C/m" cdot "1.56 m"#

#= color(blue)ul(102.396^@ "C")#

What was the change in boiling point?