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Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates...

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 25.65 mL of 0.3000 M NaOH solution to titrate both acidic protons in 60.00 mL of the tartaric acid solution. Calculate the molarity of tartaric acid and write a net ionic equation for the reaction.

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Answer #1

Tartaric acid is diprotic acid. Let us represent it as . The neutralisation reaction is

Tartaric acid is a weak acid. It is incompletely ionized. NaOH and disodium tartarte are strong electrolytes. They are completely ionised.

The net ionic equation is

Number of millimoles of NaOH are obtained by multiplying molarity with volume in mL.

Number of millimoles of NaOH  

When number of millimoles of NaOH are divided with 2, the number of millimoles of tartaric acid are obtained.

The number of millimoles of tartaric acid

The volume of tartaric acid solution is 60.00 mL. When number of millimoles of tartaric acid is divided with its volume (in mL), the molarity of tartaric acid solution is obtained.

Molarity of tartaric acid solution is

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