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

2b2t

explanation:

2b2t

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.