Problem: Two beakers are placed in a sealed box at 25 oC. One beaker contains 35.0 mL of a 5.5×10−2 M aqueous solution of a nonvolatile nonelectrolyte. The other beaker contains 35.0 mL of a 4.0×10−2 M aqueous solution of NaCl. The water vapor from the two solutions reaches equilibrium.What is the volume in the beaker with the aqueous solution of a nonvolatile nonelectrolyte when equilibrium is attained, assuming ideal behavior?

FREE Expert Solution

We are asked to determine the volume in the beaker with the aqueous non-electrolyte solution when equilibrium is attained (i.e. assuming ideal behavior)

Recall the formula for molarity:

Molarity(M)=moles solute (mol)litre solution (L)


At equilibrium

molarity NaCl=molarity non-electrolyte solution

Let x be the volume transferred from the non-electrolyte solution to the NaCl solution, therefore: 

Volume of non-electrolyte solution: 35-x

Volume of NaCl solution: 35+x


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Problem Details

Two beakers are placed in a sealed box at 25 oC. One beaker contains 35.0 mL of a 5.5×10−2 M aqueous solution of a nonvolatile nonelectrolyte. The other beaker contains 35.0 mL of a 4.0×10−2 M aqueous solution of NaCl. The water vapor from the two solutions reaches equilibrium.

What is the volume in the beaker with the aqueous solution of a nonvolatile nonelectrolyte when equilibrium is attained, assuming ideal behavior?

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