In: Chemistry
Fill in the blanks in the table. Aqueous solutions are assumed.
Compound | Molality | Weight percent | Mole Fraction |
NaI | 0.15 | ||
C2H5OH | 5.0 | ||
C12H22O11 | 0.15 |
NaI: Molality= 0.15
Amount of NaI present in 1000 gm water
= 0.15 moles
= 0.15 moles *149.89 g/mol
= 22.4835 g
1000 gm water = 1000/18 = 55.55 moles of water
So, moles fraction of NaI = 0.15/(0.15+55.55) = 2.69*10-3
Weight %
= [weight of ethanol in 1000 g water /(weight of total solution) ] * 100
= [22.4835/(1000 + 22.4835) ] * 100
= 2.20 %
C2H5OH : Weight percent of solution = 5 %
So 1000 gm solution contains 50 g ethanol.
(1000-50) or 950 g water is mixed with 50 g ethanol.
50 g ethanol = 50g/(46 g/mol) = 1.087 moles of ethanol
950 g water contains 1.087 moles of ethanol
1000 g water contains 1.087*1000/950 or 1.144 moles of ethanol.
Molality = 1.144
mole fraction of ethanol= 1.144/(55.55+1.144) = 0.020
C12H22O11 : Molality= 0.15
Amount of C12H22O11 present in 1000 gm water
= 0.15 moles
= 0.15 moles *342 g/mol
= 51.3 g
1000 gm water = 1000/18 = 55.55 moles of water
So, moles fraction of NaI = 0.15 /(0.15+55.55)
= 2.69*10-3
Weight %
= [weight of C12H22O11 in 1000 g water /(weight of total solution) ] * 100
= [51.3/(1000 + 51.3) ] * 100
= 4.88 %