Question #66b16
1 Answer
Explanation:
Assuming that you're dealing with a non-volatile solute, you can say that the vapor pressure of the solution,
#color(blue)(ul(color(black)(P_"sol" = chi_"water" * P_"water"^@)))" "color(darkorange)("(*)")#
Now, the mole fraction of water is defined as the ratio between the number of moles of water and the total number of moles present in the solution.
If you take
#m color(red)(cancel(color(black)("g"))) * "1 mole solute"/(60color(red)(cancel(color(black)("g")))) = (m/60)# #"moles solute"#
and
#180 color(red)(cancel(color(black)("g"))) * ("1 mole H"_2"O")/(18.015color(red)(cancel(color(black)("g")))) = "9.992 moles H"_2"O"#
The total number of moles in the solution will be equal to
#(m/60)color(white)(.)"moles" + "9.992 moles" = ((m + 599.52)/60)# #"moles"#
The mole fraction of water will thus be
#chi_"water" = (9.992 color(red)(cancel(color(black)("moles"))))/(( (m + 599.52)/60)color(red)(cancel(color(black)("moles")))) = 599.52/(m + 599.52)#
You know that the vapor pressure of the solution must be
#P_"sol" = 4/5 * P_"water"^@#
Plug this into equation
#4/5 * color(red)(cancel(color(black)(P_"water"^@))) = chi_"water" * color(red)(cancel(color(black)(P_"water"^@)))#
This is equivalent to
#599.52/(m + 599.52) = 4/5#
Solve for
#4 * (m + 599.52) = 599.52 * 5#
#m = (599.52 * 5 - 599.52 * 4)/4#
#m = 599.52/4 = 149.88#
Therefore, you can say that the mass of the solute is equal to
#color(darkgreen)(ul(color(black)("mass solute = 150 g")))#
I'll leave the answer rounded to two sig figs.