When 2.06 g of a nonelectrolyte solute is dissolved in water to make 505 mL of solution at 26 °C, the solution exerts an osmotic pressure of 963 torr. What is the molar concentration of the solution?

The molar concentration of the solution is 0.05162 M

Explanation:

Step 1: Data given

Mass of the nonelectrolyte solute = 2.06 grams

Volume = 505 mL = 0.505 L

Temperature = 26 °C = 299 K

Osmotic pressure =963 torr

Step 2: Calculate the molar concentration

π = i*M*R*T

⇒π = the osmotic pressure = 963 torr = 1.26711 atm

⇒i = the van't Hoff factor = for a nonelectrolyte = 1

⇒M = the molar concentration = TO BE DETERMINED

⇒R = the gas constant = 0.08206 L*atm/mol*K

⇒T = the temperature = 299.15 K

M = π / (R*T)

M = 1.26711 / (0.08206*299.15)

M = 0.05162 M

The molar concentration of the solution is 0.05162 M

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.