Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines, and a salt derived from the acid precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 24.65 mL of 0.2500 M NaOH solution to titrate both acidic protons in 50.00 mL of the tartaric acid solution. Calculate the molarity of the tartaric acid solution.

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Identify the balanced chemical equation for the reaction: \( \text{H}_2\text{C}_4\text{H}_4\text{O}_6 + 2\text{NaOH} \rightarrow \text{Na}_2\text{C}_4\text{H}_4\text{O}_6 + 2\text{H}_2\text{O} \).

Determine the moles of NaOH used in the titration: \( \text{moles of NaOH} = \text{Volume (L)} \times \text{Molarity (M)} \).

Use the stoichiometry of the balanced equation to find the moles of tartaric acid: Since 2 moles of NaOH react with 1 mole of tartaric acid, divide the moles of NaOH by 2.

Calculate the molarity of the tartaric acid solution: \( \text{Molarity} = \frac{\text{moles of tartaric acid}}{\text{Volume of tartaric acid solution (L)}} \).

Convert the volume of tartaric acid solution from mL to L by dividing by 1000, and use this in the molarity calculation.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant, a solution of known concentration, to a sample until the reaction reaches its endpoint, indicated by a color change or a specific measurement. In this case, NaOH is the titrant used to neutralize the acidic protons in tartaric acid.

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is a crucial concept in chemistry for calculating how much of a substance is present in a given volume of solution. In this problem, the molarity of tartaric acid can be determined by using the volume and molarity of the NaOH solution used in the titration.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It allows chemists to predict the amounts of substances consumed and produced in a reaction. In this scenario, understanding the stoichiometric relationship between tartaric acid and NaOH is essential to calculate the molarity of the tartaric acid solution, as each mole of tartaric acid reacts with a specific amount of NaOH.

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