Asked by cici
a solution was prepared by mixing ethanol (CH3CH2OH / d= 0.775 g/ml) with 350ml of water (H20 / d= 0.9940326). Assuming volumes were additive, determine the molarity of the solution knowing the mole fraction of water is 0.853.
help me resolve this please
help me resolve this please
Answers
Answered by
DrBob222
Remember mass = volume x density and mols = grams/molar mass
XH2O = 0.853 = (mols H2O)/[(mols H2O + mols EtOH)]
0.853 = (g H2O/18)/[(g H2O/18) + (g EtOH/46)]
0.853 = (0.994*350/18)/[(0.994*350) + (0.775*V)/46]
The only unknown is V = volume of EtOH used. Solve for that.
Then 0.775 V/46 gives you mols EtOH, then mols EtOH/total volume in L give you molarity of EtOH. Post your work if you get stuck.
XH2O = 0.853 = (mols H2O)/[(mols H2O + mols EtOH)]
0.853 = (g H2O/18)/[(g H2O/18) + (g EtOH/46)]
0.853 = (0.994*350/18)/[(0.994*350) + (0.775*V)/46]
The only unknown is V = volume of EtOH used. Solve for that.
Then 0.775 V/46 gives you mols EtOH, then mols EtOH/total volume in L give you molarity of EtOH. Post your work if you get stuck.
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