A chemistry student weighs out of ascorbic acid , a diprotic acid, into a volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with solution. Calculate the volume of solution the student will need to add to reach the final equivalence point. Round your answer to significant digits.

14.3 mL  

Explanation:

Assume the student used 0.113 g ascorbic acid  and 0.0900 mol·L⁻¹ NaOH.

1. Balanced chemical equation.

The formula of ascorbic acid is H₂C₆H₆O₆ (MM = 176.12 g/mol).

However, for the balanced equation, let's write it as H₂A.

2. Moles of ascorbic acid

3. Moles of NaOH

The molar ratio is 2 mmol NaOH:1 mmol H₂A.

4. Volume of NaOH

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