Problem: Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 23.65 mL of 0.3000 M NaOH solution to titrate both acidic protons in 55.00 mL of the tartaric acid solution.Calculate the molarity of the tartaric acid solution.

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FREE Expert Solution

Balanced equation: H2C4H4O6(aq) + 2 NaOH(aq) → Na2C4H4O6(aq) + 2 H2O(l)

  • diprotic  donates 2 H+
  • H2C4H4O 2 H+ C4H4O6-


Recall that the point where acid gets completely neutralized by a base is called equivalence point of a titration, where:


moles acid=moles base


Also, recall that moles = molarity × volume

This means:


MVacid=MVbase

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Problem Details

Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 23.65 mL of 0.3000 M NaOH solution to titrate both acidic protons in 55.00 mL of the tartaric acid solution.

Calculate the molarity of the tartaric acid solution.

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Based on our data, we think this problem is relevant for Professor Dixon's class at UCF.