What is the molar mass of the unknown?

  • Thread starter huybinhs
  • Start date
  • #1
230
0

Homework Statement



A 1.40 g sample of an unknown is dissolved in 8.10 g of lauric acid. The freezing point is depressed 1.23 oC. What is the molar mass of the unknown?



Homework Equations



Delta T = Kf * m



The Attempt at a Solution



Delta T = Kf * m
=> m = 1.23 / 3.9 = 0.32

mole solute = 0.32 * 0.0081 = 0.0026 moles.

=> Molar mass = 1.40 / 0.0026 = 540 g/mol = final answer.

Am I doing correct? Please let me know!
 

Answers and Replies

  • #2
Borek
Mentor
28,805
3,297
Not bad. Two thngs that will make your solution better.

1. Don't round down intermediate results (check that it changes molar mass by about 8g).
2. Don't ignore units in your calculations, they are much easier to follow when it is obvious what is what of what.
 
Last edited by a moderator:
  • #3
230
0
Not bad. Two thngs that will make your solution better.

1. Don't round down intermediate results (check that it changes molar mass by about 8g).
2. Don't ignore units in your calculations, they are much easier to follow when it is obvious what is what of what.

--
chemical calculators - buffer calculator, concentration calculator
www.titrations.info - all about titration methods

Thanks so much for your response!

I have edited my answer to:

Delta T = Kf * m => m = 1.23 / 3.9 = 0.32 m

mole solute = 0.32 * 0.0081 = 0.0026 mole

Molar mass of the unknown = 1.40 / 0.0026 = 538.46 g/mol .

Hope it better ;)
 
  • #4
Borek
Mentor
28,805
3,297
This time you overdid - you don't have enough information to give 5 significant digits in the answer :smile: But you see that rounding errors were responsible for 538 being 530.
 
Last edited by a moderator:

Related Threads on What is the molar mass of the unknown?

  • Last Post
Replies
1
Views
19K
Replies
1
Views
15K
  • Last Post
Replies
2
Views
52K
  • Last Post
Replies
3
Views
6K
Replies
2
Views
10K
Replies
5
Views
31K
  • Last Post
Replies
1
Views
3K
  • Last Post
Replies
3
Views
6K
Top