Ascorbic acid (vitamin C) is oxidized by iodine according to the equation below:1 mol ascorbic acid + 1 mol iodine1 mol dehydroascorbic acid + 2 mol hydroiodicacida) An iodine solution of unknown concentration is used to titrate 10.00 mL of0.003013 M ascorbic acid. If 27.55 mL of iodine is required to reach the endpoint,what is the concentration of the iodine solution? Express as a decimal.

Given: Iodine solution 10.00 ml Iodine solution of 27.55 ml required to reaction endpoint ascorbic acid=0.003013 MFormula used: No of moles of iodine=Molar concentration of iodine×volume of iodine. Number of moles of ascorbic acid=0.0030313×101000 =0.0303131000 Where 1 mole of ascorbic acid +1 mole iodine gives 1-mole dehydroascorbic acid+2 mole hydroiodic acid 0.0303131000 of ascorbic acid react with 0.0303131000 of iodine so, No of moles of iodine=Molar concentration of iodine×volume of iodine. 0.0303131000=Molar concentration of iodine×27.551000 On solving, The molar concentration of iodine=0.0011002 M

Answered: Ascorbic acid (vitámin C) is oxidized…