Question #7d76d

1 Answer
Jul 24, 2016

Answer:

Here's what I got.

Explanation:

Interestingly enough, you don't need to know the density of the solution to calculate its molality and the mole fraction of hydrochloric acid, #"HCl"#, your solute.

All you need to know here is the solution's mass by mass percent concentration, #"% m/m"#, which is said to be equal to #36%#.

Now, to make the calculations easier, pick a sample of this solution that has a mass of #"100 g"#. According to the given percent concentration, this sample will contain

  • #"36 g"# of hydrochloric acid
  • #"64 g"# of water

Use the molar masses of hydrochloric acid and of water to determine how many moles of each you have in this sample

#36 color(red)(cancel(color(black)("g"))) * "1 mole HCl"/(36.46color(red)(cancel(color(black)("g")))) = "0.9874 moles HCl"#

#64 color(red)(cancel(color(black)("g"))) * ("1 mole H"_2"O")/(18.015color(red)(cancel(color(black)("g")))) = "3.553 moles H"_2"O"#

The mole fraction of hydrochloric acid, #chi_"HCl"#, is defined as the number of moles of acid divided by the total number of moles present in solution.

In your case, you will have

#chi_"HCl" = (0.9874 color(red)(cancel(color(black)("moles"))))/((0.9874 + 3.553)color(red)(cancel(color(black)("moles")))) = color(green)(|bar(ul(color(white)(a/a)color(black)(0.22)color(white)(a/a)|)))#

Next, the molality of th solution is defined as the number of moles of solute divided by the mass of solvent expressed in kilograms. In your case, the molality of the solution will be

#b = "0.9874 moles"/(64 * 10^(-3)"kg") = "15.4 mol kg"^(-1)#

I'll round this off to two sig figs, the number of sig figs you have for the solution's percent concentration.

#b = color(green)(|bar(ul(color(white)(a/a)color(black)("15 mol kg"^(-1))color(white)(a/a)|)))#