A 40.00-mL sample of 0.0500 M HNO2 is titrated with 0.0200 M Cs4+. The pH is held constant at 0. The potential is measured relative to the calomel electrode (E=0.241 V). a. Write out the two ½ reactions, the net reaction and the Nernst equation in general form for this titration before the equivalence point.
b. What is the potential at the equivalence point and 2Ve (two times the volume required to reach the equivalence point)?
c. What is the potential at the equivalence point, if an AgCl electrode (E=0.199) is used as a reference electrode?
d. What indicator could be used to measure the endpoint for this titration?

is that all the question

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.