In a vitamin C analysis, triiodide ions are generated in solution by the following unbalanced reaction in acidic solution:
IO3- (aq) + I- (aq) --> I3- (aq)
I2- is determined by titration with Na2S2O3 solution. The products are (I-) and (S4O62-).
a) Balance the equation for the half reaction of IO3- (aq) with I- ions.
b) A sample of 0.6013 g of KIO3 was dissolved in water; HCL and sodium potassium iodide were then addeed in excess. What is the minimum weight of solid KI and the minimum volume of 3.00 M HCL required to convert all of the IO3- ions to I3- ions?
c) Write and balance the stoichiometric equation for the reaction of S2O32- with I3- in acidic solution.
Totally lost on these redox equation
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1) to balance half reactions you need to consider acidity of the solutions.
Unbalanced:
IO3-(aq) + I-(aq) + H+ = I3-(aq) + H2O
Balanced:
http://www.webqc.org/balance.php?reacti ... q%29%2BH2O
2)
Unbalanced:
2 S2O32- + I3- = S4O62- + 3 I-
Balanced:
http://www.webqc.org/balance.php?reacti ... 2BI%7B-%7D
Can you solve this problem now? Let me know if not.
J. Mac
Unbalanced:
IO3-(aq) + I-(aq) + H+ = I3-(aq) + H2O
Balanced:
http://www.webqc.org/balance.php?reacti ... q%29%2BH2O
2)
Unbalanced:
2 S2O32- + I3- = S4O62- + 3 I-
Balanced:
http://www.webqc.org/balance.php?reacti ... 2BI%7B-%7D
Can you solve this problem now? Let me know if not.
J. Mac