# If I pass dry air through solutions of 0.1 mol/L KCl and 6 mol/L HCl, which solution will lose mass?What will happen if I use moist air instead?

Mar 29, 2015

Some water of the first solution will evaporate into the dry air.

The more concentrated the solution, the more it will 'stick' to the water it's dissolved in.

The 6M solution will thus absorb a great part of the water vapour that came from the first solution. A small part of the second solution will evaporate, but not as much as was taken in.

Evaporation depends on the concentration of solvents.

Mar 29, 2015

Actually, both solutions will lose mass.

#### Explanation:

Dry Air

There is no moisture in dry air, so the partial pressure of the water is zero.

0.1 mol/L $\text{KCl}$

The vapour pressure of pure water at 20°C is 2.4 kPa.

The dissolved KCl will reduce this slightly, perhaps to about 2.0 kPa.

When you pass dry air through the solution, water molecules will move into the dry air.

The $\text{KCl}$ solution will lose mass.

6 mol/L $\text{HCl}$

In 6 mol/L $\text{HCl}$, the vapour pressure of water is less than 2 kPa, but the partial pressure of hydrogen chloride gas more than compensates for this.

${P}_{\text{H₂O" + P_"HCl" = "14 kPa}}$

As you pass the moist air through the $\text{HCl}$, some water will move into the $\text{HCl}$.

But more hydrogen chloride will move into the air stream, and the $\text{HCl}$ solution will have a net loss of mass.