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.Write a balanced net ionic equation for the neutralization reaction.

FREE Expert Solution

The reaction of H2C4H4O6 with NaOH is as follows:

H2C4H4O6(aq) + NaOH(aq) → Na2C4H4O6(aq) + H2O(l)

To balance this, we add a coefficient of 2 to NaOH and H2O. The molecular equation for the neutralization reaction is:

H2C4H4O6(aq) + 2 NaOH(aq) → Na2C4H4O6(aq) + 2 H2O(l)

To get the total ionic equation, split the soluble ionic compounds into the constituent ions. Tartaric acid isn't split since it's a weak acid:

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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.

Write a balanced net ionic equation for the neutralization reaction.

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