What is the molarity of a solution prepared from 10.0 grams of methanol (ch3oh, density = 0.792 g/ml) with 125.0 milliliters of ethanol (ch3ch2oh)? assume the volumes are additive.

Molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.

The molarity of a solution is calculated according to the following formula:

molarity= moles÷ volume

Molarity is expressed in units [tex]\frac{moles}{L}[/tex].

This case

In this case, you have for methanol:

Mass= 10 g
Density= 0.792 g/mL
Volume= mass÷ density= 10 g÷ 0.792 g/mL= 7.92 mL
Molar mass= 32 g/mol
Moles of methanol= mass÷ molar mass= 10 g÷ 32 g/mole= 0.3125 moles

On the other hand, you know for ethanol:

Volume= 125 mL

Assuming additive volumes, the total volume is:

Total volume= Volume methanol + Volume ethanol= 7.92 mL + 125 mL= 132.92 mL= 0.13292 L (being 1000 mL= 1 L)

Replacing in the definition of molarity:

molarity= moles of methanol÷ total volume

molarity= 0.3125 moles÷ 0.13292 L

Solving:

molarity= 2.351 [tex]\frac{moles}{L}[/tex]= 2.351 M

Finally, the molarity of the solution is 2.351 M.

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