Achemistry student weighs out 0.0475g of sulfurous acid h2so3, a diprotic acid, into a
250.ml volumetric flask and dilutes to the mark with distilled water. he plans to titrate the acid with 0.1100m naoh solution.

calculate the volume of naoh solution the student will need to add to reach the final equivalence point. be sure your answer has the correct number of significant digits.

The volume of NaOH required is 10.5 mL

Explanation:

To calculate the molarity of solution, we use the equation:

Mass of solute (sulfurous acid) = 0.0475 g

Molar mass of sulfurous acid = 82 g/mol

Volume of solution = 250. mL

Putting values in above equation, we get:

where,

are the n-factor, molarity and volume of acid which is

are the n-factor, molarity and volume of base which is NaOH.

We are given:

Putting values in above equation, we get:

Hence, the volume of NaOH required is 10.5 mL

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.