Final answer:
In a redox titration, the number of moles of citric acid present in the sample is also 2.354×10⁻⁵ moles.
Step-by-step explanation:
In a redox titration, the amount of ascorbic acid in a sample is determined by oxidizing the ascorbic acid to dehydroascorbic acid with a known amount of iodide ion (I-), and then back titrating the excess iodide ion with sodium thiosulfate (Na₂S₂O₃).
From the given information, we know that the 10.00 ml sample contained 2.354×10⁻⁵ moles of ascorbic acid.
We can use the balanced equation for the reaction between ascorbic acid (C₆H₈O₆) and iodide ion (I⁻) to find the mole ratio between ascorbic acid and iodide ion.
The balanced equation is:
2C₆H₈O₆ + I₂ --> 2C₆H₆O₆ + 2I⁻
From the equation, we can see that 2 moles of ascorbic acid react with 1 mole of iodide ion.
Therefore, the number of moles of iodide ion consumed in the reaction is also 2.354×10⁻⁵ moles.
To find the number of moles of citric acid, we need to use the mole ratio between ascorbic acid and citric acid.
The balanced equation for the reaction between citric acid (C₆H₈O₇) and iodide ion (I⁻) is:
C₆H₈O₇ + 2I₂ --> C₆H₆O₇ + 4I⁻
From this equation, we can see that 1 mole of ascorbic acid reacts with 1 mole of citric acid.
Therefore, the number of moles of citric acid in the sample is also 2.354×10⁻⁵moles.