chemistry

The freezing point of a 0.010 m aqueous solution of a nonvolatile solute is ?0.072°C. What would you expect the normal boiling point of this same solution to be?

have no clue, thanks for the thelp


Freezing point depression= N*kf* molality

you have freezing point depression, molality, and you know kf for water. Calculate N

Then:
bp = 100 + N*kb*m

yes, thanks al ot

  1. 0
  2. 0
  3. 13
asked by tyler
  1. First you solve for I (vant hoff factor) in the freezing point eqn. You are provided molality, delta fp and can get the kf from a textbook (hint since its aqueous, use value for h2o).

    Next, take this I value and plug it into the boiling point eqn with the given molality and the kb value from the text for h2o to solve for delta bp. Add 100 degrees (waters boiling point)

    1. 0
    2. 0
    posted by erin

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute

    asked by Allie on February 19, 2016
  2. chemistry

    1. Would it be advisable to determine the freezing point of pure p-dichlorobenzene with one thermometer and the freezing point of the solution with a different one? Explain. 2. If 0.150 mole of a nonvolatile non-electrolyte solute

    asked by Larry on February 2, 2012
  3. chemistry

    I need help on these questions. They all seem pretty similar i think? i don't know what formula i am suppose to use. And what does nonvolatile mean? is that like a clue or something? 1) 2.6 g of the nonvolatile solute sucrose

    asked by confusedkid on January 25, 2009
  4. Physical Chemistry

    When 1.33 g of a nonpolar solute was dissolved in 50.0 g of phenol, the latter's freezing point was lowered by 1.454°C. Calculate the molar mass of the solute. The kf of phenol is 7.27 (K·kg)/mol. What is the normal boiling

    asked by Anonymous on May 24, 2010
  5. Chemistry

    What effect do each of these have on the freezing point of the solvent? a. a nonvolatile solute that dissociates in the solvent b. a volatile solute that does not dissociate c. two solutes that react according to the equation:

    asked by Sylvia on June 23, 2009
  6. Physical Chemistry

    When 3.78 g of nonvolatile solute is dissolved in 300.0 g of water, the freezing point depression is 0.646 o C. Calculate the molar mass of the solute. The cryoscopic constant of water is 1.86 K kg mol -1. When 3.78 g of

    asked by Lan on October 12, 2006
  7. chemistry

    A freezing point depression experiment was conducted using cyclohexane as the solvent. The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point of a solution

    asked by Danielle on February 16, 2015
  8. chemistry

    which of the following liquids have the highest freezing point? a- aqueous Fe(NO3)3 (0.030) b- aqueous glucose (0.050 m) c- aqueous NaI (0.030 m) d- aqueous NaI (0.010 m) e- pure water please explain the concept behind it as well

    asked by Ania on November 6, 2012
  9. Chem(again)

    What is the relationship between the amount of solute and the amount of freezing point depression? delta T = kf m where delta T is the difference between the normal freezing point and the f.p. with a solute, kf is the freezing

    asked by Chrissy on February 6, 2007
  10. chemistry

    A compound was found to be composed of the following amounts of elements: 20.00% wt% C, 26.64wt% O, 46.65 wt%N, and 6.71wt%H. A 6.125 grams sample of this compound dissolved in 46.205 grams of water as a solution was found to have

    asked by lucy on April 25, 2013

More Similar Questions