A 0.629 g sample of a diprotic acid is dissolved in water and titrated with 0.270 M NaOH. What is the molar mass of the acid if 36.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. A flask with a solution sits on the base of a ring stand. A buret filled with liquid is suspended above the flask by the ring stand. molar mass: g/mol

The molar mass of acid is 127.97 g/mol

Explanation:

To calculate the number of moles for given molarity, we use the equation:

Molarity of NaOH solution = 0.270 M

Volume of solution = 36.4 mL

Putting values in above equation, we get:

The chemical equation for the reaction of NaOH and diprotic acid follows:

By Stoichiometry of the reaction:

2 moles of NaOH reacts with 1 mole of diprotic acid

So, moles of diprotic acid =

To calculate the number of moles, we use the equation:

Mass of acid = 0.629 g

Moles of acid = 0.004915 moles

Putting values in above equation, we get:

Hence, the molar mass of acid is 127.97 g/mol

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.

quartz

explanation: