What is the osmotic pressure of a 0.25 M solution of NaCl at 25 degrees C? can s

Question

What is the osmotic pressure of a 0.25 M solution of NaCl at 25 degrees C?

can someone show me how to solve this and give me the correct answer please

Explanation / Answer

Let XY dissolve according to XY(s) ? X?(aq) + Y?(aq) Hence : Ksp = [X?]·[Y?] Let the solution be saturated, so that it contains apparently M moles of XY dissolved per liter of solution. Assuming complete dissociation the ionic molarities in the solution are: [X?] = [Y?] = M => Ksp = M² The apparent molarity of the solution can be found from the osmotic pressure. The osmotic pressure of a dilute solution is given by Morse equation : p = i·R·T·M i is the van't Hoff factor of solution. It describes the number of particles formed per molecule dissolved . Her we got 2 ions per salt molecule, i.e. i=2 R = 8.3145Pam³/molK = 62.363?67torrL/molK [3]is the universal gas constant T absolute temperature Hence: M = p / (i·R·T) = 45.6torr / (2 · 62.363?67torrL/molK · 298.15K) = 1.226×10?³mol/L => Ksp = (1.226×10?³)² = 1.50×10?6

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