Use the Henderson- Hasselbalch equation to calculate the pH of
each solution.
a. a solution that is 0. 145 M in propanoic acid and 0. 115 M in
potassium propanoate
b. a solution that contains 0.785% C5H5N by mass and
0.985% C5H5NHCI by mass
c. a solution that contains 15.0 g of HF and 25.0 g of NaF in
125 mL of solution

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.

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explanation:

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