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:

For sulfurous acid:

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:

To calculate the volume of base, we use the equation given by neutralization reaction:

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

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