ap chemistry

what would have happened to your calculated molar mass if some lauric acid was spiled before finding the freezing point?

  1. 0
  2. 0
  3. 6
asked by de
  1. help please?

    1. 0
    2. 0
    posted by de
  2. (1)delta T = Kf*m
    Substitute delta T and Kf; solve for m

    (2)m = mols/kg solvent
    Substitute m and kg solvent; solve for mols

    (3)mols = grams/molar mass. Rearrange to molar mass = grams/mols.

    Now follow through with equation 1, 2, and 3.

    If some of the lauric acid (but you have weighed a larger amout) is apilled delta T in 1 will be too small because you have too little to begin with. That makes m too small since k is a constant; i.e., m = delta T/Kf.

    Too small m in equation 2 gives mols that is too small since mols = m x kg solvent; since m is too small then m x kg solvent will be too small.

    Then go to equation 3. This one (rearranged form) is
    molar mass = grams/mol. If you have mols too small that gives a molar mass that is too large. So your calculated molar mass is too large.

    1. 0
    2. 0
    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. ap chemistry

    what would have happened to the calculated molar mass if some benzoic acid was spilled before adding it to the lauric acid? also, what would have happened to the calculated molar mass if the thermometer used actually read 1.4C too
  2. chemistry

    A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300g instead of8.003g. The calculated molar mass of the unknown acid will be GREATER/LESS
  3. chemistry

    (A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g instead of 8.003 g. The calculated molar mass of the unknown acid will be
  4. chemistry

    A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass of lauric acid as 8.300 g instead of 8.003 g. The calculated molar mass of the unknown acid will be
  5. chemistry

    1) The color of bromocresol green indicator is??? when pH < 4, green when pH 4- 5.3 and ???? in pH > 5.3. 2)(A) A student performed the freezing point depression experiment according to directions but mistakenly recorded the mass
  6. lauric acid

    what happens to the calculated molar has if the lauric acid is spilled before determining the freezing point?
  7. Chemistry

    Calculate the expected freezing point of a solution of 0.579 g pelargonic acid in 4.225 g of lauric acid, if the melting point of pure lauric acid was measured to be 43.20*C. (MM pelargonic acid = 158.2 g/mol; MM laruic acid =
  8. APChem

    If an air bubble passes unnoticed through the tip of a buret during a titration (where a weak nonvolatile acid HA is the analyte) , the calculated molar mass of HA would be too high, too low, or not affected? I thought it would be
  9. Chemistry h/w

    Hi, this is my first lab in 2nd semester of chemistry, and im not sure about my answers in the assignment can someone give it a quick look to check them? this is my phase diagram: tinypic. com/view.php?pic=1605yev&s=7 p.s. ignore
  10. chemistry h/w

    Hi, this is my first lab in 2nd semester of chemistry, and im not sure about my answers in the assignment can someone give it a quick look to check them? this is my phase diagram: tinypic. com/view.php?pic=1605yev&s=7 p.s. ignore

More Similar Questions