A solution contains 0.182 molmol NaClNaCl and 0.897 molH2OmolH2O. Calculate the vapor pressure of the solution at 55 ∘C∘C. The vapor pressure of pure water at 55 ∘C∘C is 118.1 torrtorr. (Assume that the solute completely dissociates.)

Vapor pressure of solution is 78.2 Torr

Explanation:

This is solved by vapor pressure lowering:

ΔP = P°. Xm. i

Vapor pressure of pure solvent (P°) - vapor pressure of solution = P°. Xm. i

NaCl → Na⁺ + Cl⁻ i = 2

Let's determine the Xm (mole fraction) These are the moles of solute / total moles.

Total moles = moles of solvent + moles of solute

Total moles = 0.897 mol + 0.182 mol → 1.079 mol

0.182 / 1.079 = 0.168

Now we replace on the main formula:

118.1° Torr - P' = 118.1° Torr. 0.168. 2

P' = - (118.1° Torr. 0.168. 2 - 118.1 Torr)

P' = 78.2 Torr