If you are lucky enough to find an OTC product that lists the contents more often then not they are in % composition. I used to think I could do the
conversion fairly well, however during my recent excursion into HBr manufacture my figures for the molarity of the solution (48%) thus resulting were
off by an unacceptable amount.
Therefore I ask three questions, beginning questions, assume I have no prior ability:
How would I find the molarity of a 48% solution of HBr in H2O? (Yes, I know the answer but I want to see how others found it).
How would I find the molarity of a 6% NaOCl solution? (I know this one too but wanted a solid dissolved in water to make this question more
complete).
And to round off the common states of matter, the molarity of a 70% isopropyl alcohol solution in water.
And what's up with the w/w and w/v aspects. Seriously, I never learned any of this in chemistry, everything was always in
molarity and it was unheard of to have a percent solution, therefor my current techniques are a mishmash of internet help sites that somehow produce
reasonable numbers.
Yes, I have googled my butt of on this one, and because this is in the beginnings section I'm hopping, no, pleading, for a bit of spoon feeding
DDTea - 17-6-2004 at 20:01
I have found that percentages are done by mass and not volume; at least from my experience with 30% Nitromethane. So, naturally, it's just
making percentage calculations for a given mass... For example, 30% of 100 g of NM solution is 30 g... At least, such calculations worked for the
Chloropicrin synthesis, so I'm assuming I've done this properly. If, however, it is done by volume, naturally you will find the percent of
a given volume, then look up the density of the given chemical to find the mass.
molarity vs %
Magpie - 17-6-2004 at 21:18
Samosa is correct but I will approach this a little differently:
Molarity is g-moles per liter of solution.
For consumer products gases and solids are usually reported in wt%. For liquids in solution it will likely be vol%.
Assuming, for the sake of argument, that HBr is a liquid, then molarity would be:
molarity = [(vol% HBr/100)(vol of soln, mL)(sp. gr. of HBr)/(MW of HBr)]/[vol of soln, L]
- this assumes no volume change on mixing.
For 6% NaOCl,
molarity = [(wt% NaOCl/100)(wt of soln, g)/(MW HBr)]/[vol of soln, L].
Hope this helps and that I didn't just add to the confusion.Proteios - 18-6-2004 at 08:09
chemists tend to like
molarity.....moles per litre of SOLUTION
-good for volumetric chemistry
physists like
molality.... moles per kilo (in the case of water 1l) of SOLVENT
-good if you are dealing with masses, not volumes.
for concentrations up to about 3-5M there really isnt much difference between the two......the 6% bleach soln. will almost be exactly the same in
molality as molarity. However for the 70 % IPA its actually more sensible to deal with mole fractions/ molality.
1kilo of solution contains
700 g IPA, 300g water
3.333x700 g IPA: 1kg H2O
xmoles IPA: ymoles H2O
The problem with the convertion to molarity is you will need the density of the solution.... and thats a function of concentration. Mole fraction and
molal is a far easier way to go in all but volumetric chemsitry.The_Davster - 18-6-2004 at 16:45
When calculating the molarity of the 6% sodium hypochlorite solution why did you divide by the molar weight of HBr, or is that a typo?
So a 10.8% sodium hypochlorite solution would work out to what? I need this so I can run the stoich and calculate my yield for the haloform reaction.
Edit: I actually got off my lazy ass and got some numbers. I did two trials because I was using a 50mL graduated cylinder for volume
measurements(could not find my 10mL pipett).
Trial 1 v=10.0 mL m=11.4g
Trial 2 v=1.00mL m=10.7g
ave mass per 10 mL=12.05g...hmm those numbers are too different mabey I should have shook the bleach up first?
so c=((10.8%)/(100%))(12.05g))/((74.44g/mol)(0.0100L))
c=1.75mol/L
Does that sound right to everyone?
[Edited on 19-6-2004 by rogue chemist]
molarity calculation
Magpie - 18-6-2004 at 18:10
rogue chemist:
1) You divide the weight of the solute (HBr or NaOCl) in grams by the molecular weight. This gives you the number of g-moles that you have. This is
necessary no matter what the solute.
2) Your calculation looks good to me.
meh
Magpie - 18-6-2004 at 18:12
That was a typo! sorry.t_Pyro - 18-6-2004 at 19:29
The only problem I face in this regard is that not all chemical suppliers state the r.d. of the solution on the labels, printing only the %
composition. Therefore, when I try to look up the r.d.'s of the solutions (with known % compositions) from chemfinder, they very from site to
site! eg. one site listed 70% HNO<sub>3</sub> as 1.37 while another claims it is 1.42. My experimental observations agree with neither-
1.25!
Does anyone know any site which has an index of the r.d's of some common reagents along with their respective % compositions?
r.d.?
Magpie - 19-6-2004 at 08:31
I have never heard the term "r.d." but I assume it means density.
Since I am "old school" I go to Perry's "Chemical Engineer's Handbook" for densities of common reagents. I believe the
CRC handbook also has such tables. Then there is the ultimate "International Critical Tables" if you have access to a good technical
library.
There is a thread on this I believe. Search on Tom Haggen. He was looking for such a table on nitric acid IIRC.t_Pyro - 19-6-2004 at 19:11
r.d.= relative density. r.d. is the ratio of the mass of "x" volume of a solution to "x" volume of pure water at
14.5<sup>o</sup>C.
Thanks for the references- I'll look them up.eidolonicaurum - 7-1-2014 at 03:49
I had this exact same problem several years ago, and I asked my science teacher how to work it out. I got this formula:
Conc. moles = <u>known molarity x unknown percentage</u> ____________________known percentage
So to calculate the concentration of a 28% solution of sulphuric acid:
<u>18.4 x 28</u> = 5.26M __98
It does, however, require the knowledge of the percentage concentration of a known molar concentration.
[Edited on 7-1-2014 by eidolonicaurum]
[Edited on 7-1-2014 by eidolonicaurum]Zyklon-A - 7-1-2014 at 06:42
Posted in 2004....eidolonicaurum - 9-1-2014 at 01:18
It may be of use to future people who look at it. Pyro - 9-1-2014 at 03:59
my first thought is:
48% HBr means that in 100g of the acid there are 48g of HBr gas
6% NaOCl means that in 100g of solution there is 6g NaOCl
70% IPA means that in 100g of the soln. there are 70g IPA
from that you can calculate the molarity.
but after reading the replies, I'm confused...
BromicAcid - 9-1-2014 at 04:30
The real problem is that for concentrated solutions the density is affected and there is no accurate rule of thumb. Concentrated ammonia solution is
0.88 g/mL whereas concentrated hydrogen chloride solution is 1.19 g/mL. Without knowing the density it can be difficult to convert to molarity
because molarity by definition requires you to know moles per liter.
So eidolonicaurum your equation would not account for a much more or much less concentrated solution because the density is going to change so wildly
but for solutions of similar concentration it would work because using the reference you would have a nearby starting point. blogfast25 - 9-1-2014 at 06:12
