# 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.

###### 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:

Also, recall that moles = molarity × volume

This means:

$\overline{){\left(\mathbf{MV}\right)}_{{\mathbf{acid}}}{\mathbf{=}}{\left(\mathbf{MV}\right)}_{{\mathbf{base}}}}$

95% (175 ratings) ###### 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.