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

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

14 days is the half-life of phosphorus-32