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The osmotic pressure of an aqueous solution at $25$ Celsius is $92.0$ $kPa$. Calculate the boiling point of the solution. (Assume that the density of the solution is $1.0$ $g/mL$, ignore the mass of the solute)

Using the formula $\pi = cRT = \rho g h$, we can find the concentration value and height; however, how one should proceed to evaluate the boiling point using the ebullioscopic constant and morality of the solution? Are there any suggested ideas for solving it, considering all the givens are outlined in the statement?

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  • $\begingroup$ Are there any ideas except for the formula $\pi = cRT$ $\endgroup$
    – Snowflake
    May 7 at 6:51
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    $\begingroup$ Is there any information about the molar mass or molecular formula of the compound? $\endgroup$
    – M.L
    May 7 at 7:00
  • $\begingroup$ No, unfortunately. That was the part where I was stuck basically. No additional information is given. $\endgroup$
    – Snowflake
    May 7 at 7:04
  • $\begingroup$ @M.L In fact, according to the statement, it has been mentioned that the mass of the solute should be ignored. And regarding the molar mass, I guess we can find it using the $\pi = MRT$ formula. What do you think? $\endgroup$
    – Snowflake
    May 7 at 7:07
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    $\begingroup$ Not sure what the problem is--you can calculate the solute concentration from the osmotic pressure. Then you can calculate the boiling point elevation from the concentration. You don't need the molar mass, since osmotic pressure and boiling point elevation both (to first order) depend only on conentration. $\endgroup$
    – theorist
    May 7 at 9:30

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