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shyiere4068
21.09.2019 •
Chemistry
An aqueous solution is listed as being 33.8% solute by mass with a density of 1.15 g/ml, the molar mass of the solute is 145.6 g/mol and the molar mass of water is 18.0 g/mol. a) what is the molality of the solution? b) what is the mole fraction of the solute?
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Ответ:
A) 2.69 M
B) 0.059
Explanation:
A) We have:
33.8% solute by mass= 33.8 g solute/100 g solution
molarity = mol solute/ 1 L solution
molarity=
x
x
x ![\frac{1000 ml}{1 L}](/tpl/images/0250/3560/af0ff.png)
molarity= 2.69 mol solute/L solution = 2.69 M
B) We know that there are 33.8 g of solute in 100 g of solution.
As the total solution is compounded by solute+solvent (in this case, solvent is water), the mass of water is the difference between the mass of the total solution and the mass of solute:
mass of water= 100 g - 33.8 g = 66.2 g
Now, we calculate the number of mol of both solute and water:
mol solute= 33.8 g solute x
= 0.232 mol
mol H20= 66.2 g H₂O x![\frac{1 mol H2O}{18 g}](/tpl/images/0250/3560/9f964.png)
Finally, the mol fraction of solute (Xsolute) is calculated as follows:
Xsolute=![\frac{mol solute}{total mol}= \frac{mol solute}{mol solute + mol H2O}=\frac{0.232 mol}{0.232 mol + 3.677 mol}](/tpl/images/0250/3560/86a68.png)
Xsolute= 0.059
Ответ: