Solution concentration and ppm

  • #1
118
0
Hi all, I have 2 short questions, that have caused me trouble in my study.

Firstly,
What is generally considered to be a highly concentrated solution?
eg. 250mL acid in 10L water.
This is 250E-3/10 = 0.25/10 = 0.025 M.
Would that be considered a concentrated solution? as it seems very low ...


Secondly,
In a sample of ground water, iron in the form of Fe2+ was found to have concentration 9.00E-3 M. Assuming the density of water is 1.00 gmL-1, what is the concentration of Fe2+ in ppm?
Now I'm not really sure what is going on here, but given the Fe2+ has a molar concentration of 9.00E-3, surely there is a way to convert that to gL-1 and then to mg/kg (ppm solute/solvent form)?
am i correct?
(just need to be lead on the right track there ...)

cheers
Steven
 

Answers and Replies

  • #2
danago
Gold Member
1,122
4
Hi all, I have 2 short questions, that have caused me trouble in my study.

Firstly,
What is generally considered to be a highly concentrated solution?
eg. 250mL acid in 10L water.
This is 250E-3/10 = 0.25/10 = 0.025 M.
Would that be considered a concentrated solution? as it seems very low ...

Hey :smile:

To calculate the molarity of the final solution, youre going to need to know what the concentration of the original 250mL acid solution is, so you can find how many moles in the final solution.
 
  • #3
118
0
Hey sup

The question for the first part im working on doesnt actually state any other values for me to work with. It states; "Household vinegar can be produced by adding 250mL of acetic acid to 10L of pure water. Which of the following best describes the acetic acid".
The answer is; "a concentrated solution of weak acid"
Now what I worked out before (0.025M) I thought was pretty low for a high concentration.
Any ideas?
 
  • #4
118
0
part a i got fine now... just another stupid misunderstanding ....

any other suggestions for part b?
 
  • #5
danago
Gold Member
1,122
4
For the second question, you are told the concentration of Fe+2 in mol/L. You should start by converting that to a concentration in g/L, and then g/mL. See if you can go from there.
 
  • #6
118
0
Thanks for your help :)

[Fe2+]=0.009
=0.50265 g/L
=0.50265 x 10^3 mg/L
=502.65 mg/L
therefore
502.65 ppm

cheers
 
  • #7
chemisttree
Science Advisor
Homework Helper
Gold Member
3,617
638
Hey sup

The question for the first part im working on doesnt actually state any other values for me to work with. It states; "Household vinegar can be produced by adding 250mL of acetic acid to 10L of pure water. Which of the following best describes the acetic acid".
The answer is; "a concentrated solution of weak acid"
Now what I worked out before (0.025M) I thought was pretty low for a high concentration.
Any ideas?

The acetic acid referred to in the question is the glacial acetic acid used to make the more dilute vinegar (250 mL in 10L). It is essentially 100% acetic acid. Thus the 'concentrated solution of a weak acid" is the closest to the correct answer, however; it isn't really a solution at all since it is water-free. It's a pure compound.
 

Related Threads on Solution concentration and ppm

  • Last Post
Replies
3
Views
1K
Replies
8
Views
1K
Replies
6
Views
3K
  • Last Post
Replies
1
Views
2K
  • Last Post
Replies
7
Views
910
  • Last Post
Replies
17
Views
1K
  • Last Post
Replies
1
Views
2K
Replies
3
Views
6K
Replies
2
Views
1K
Replies
14
Views
10K
Top