Question

In a redox titration: only 0.275 g of pure Ascorbic acid C6H8O6 (M.wt. = 176.12 g/mol) were dissolved in 25.00 mL and required 43.50 mL of iodine to reach the end point and produce a 65.33 mL of iodide. What is the molar concentration of the iodine solution? The chemical reaction is: C6H8O6 + I2 ------> C6H6O6 + 2H+ + 2I- 0.0115 M 0.0398 M 0.0625 M 0.0359 M

          In a redox titration: only 0.275 g of pure Ascorbic acid C6H8O6 (M.wt. = 176.12 g/mol) were dissolved in 25.00 mL and required 43.50 mL of iodine to reach the end point and produce a 65.33 mL of iodide. What is the molar concentration of the iodine solution? The chemical reaction is:

C6H8O6 + I2 ------> C6H6O6 + 2H+ + 2I-

0.0115 M
0.0398 M
0.0625 M
0.0359 M

Show more…

In a redox titration: only 0.275 g of pure Ascorbic acid C6H8O6 (M.wt. = 176.12 g/mol) were dissolved in 25.00 mL and required 43.50 mL of iodine to reach the end point and produce a 65.33 mL of iodide. What is the molar concentration of the iodine solution? The chemical reaction is:

C6H8O6 + I2 ——> C6H6O6 + 2H+ + 2I-

0.0115 M
0.0398 M
0.0625 M
0.0359 M

Added by Crystal A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ronald Prasad

09/05/2023

Step 1

We can do this by dividing the mass of ascorbic acid by its molar mass: moles of C6H8O6 = (0.275 g) / (176.12 g/mol) = 0.00156 mol Now, we can find the concentration of ascorbic acid in the 25.00 mL solution: concentration of C6H8O6 = (0.00156 mol) / (0.025 L) Show more…

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In a redox titration: only 0.275 g of pure Ascorbic acid C6H8O6 (M.wt. = 176.12 g/mol) were dissolved in 25.00 mL and required 43.50 mL of iodine to reach the end point and produce a 65.33 mL of iodide. What is the molar concentration of the iodine solution? The chemical reaction is: C6H8O6 + I2 ------> C6H6O6 + 2H+ + 2I-

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