Seawater contains 3.4 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCl (over 90% is), calculate the osmotic pressure of seawater at 23°C.
By using the formula osmotic pressure=(molarity)(temperature)(R), I got this...
1. M=mol/L=(3.4/58.4)/1 [because it says per liter]
2. T=23+273=296
3. MTR=1.41
...but the answer I got was wrong, so I tried multiplying the moles by .9 (thinking the 90% part was important), but the answer was still wrong. Any ideas?
2006-12-30
08:07:00
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2 answers
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asked by
SDesign
1
in
Chemistry