Unknown number 3 determination 2 determination 1 10.00ml 19.l00ml 00.00ml 19.40ml 0.0la01m 10.00ml 20.50ml 00.00mt volume of unknown used, ml final buret reading, ml initial buret reading, ml 20.50ml volume of naoh solution used, ml molarity of naoh solution, mol/l moles of naoh, mol (show how you set up this calculation) moles of h displaced by cu2+ (show a sample calculation) moles of cu2+ on column (show a sample calculation) concentration of cu2+ in sample, mol/l (show a sample calculation) average concentration of cu2+ in sample, mol/l

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.