Calculate the total moles of triiodide added to each flask containing Vitamin C. Include the written calculation.

Steps to Solve

1. Identify the given data

We have the volume of titrant from three trials: Trial 1: 11.38 mL Trial 2: 12.46 mL Trial 3: 12.49 mL

2. Find the concentration of the triiodide solution

The concentration of the triiodide solution is needed to calculate the number of moles. Since it is not provided in the text, we will assume a concentration of 0.01 M (mol/L) for demonstration purposes. In a real experiment, this value would be known.

3. Convert volume from mL to L

To convert mL to L, divide by 1000: Trial 1: $11.38 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.01138 \text{ L}$ Trial 2: $12.46 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.01246 \text{ L}$ Trial 3: $12.49 \text{ mL} \times \frac{1 \text{ L}}{1000 \text{ mL}} = 0.01249 \text{ L}$

4. Calculate the moles of triiodide for each trial

Use the formula: $\text{moles} = \text{concentration} \times \text{volume}$ Trial 1: $\text{moles} = 0.01 \text{ M} \times 0.01138 \text{ L} = 0.0001138 \text{ moles}$ Trial 2: $\text{moles} = 0.01 \text{ M} \times 0.01246 \text{ L} = 0.0001246 \text{ moles}$ Trial 3: $\text{moles} = 0.01 \text{ M} \times 0.01249 \text{ L} = 0.0001249 \text{ moles}$

5. Summarize the results

Total moles of triiodide added: Trial 1: 0.0001138 moles Trial 2: 0.0001246 moles Trial 3: 0.0001249 moles