Chemical Concept Demonstrated: Chemical kinetics
|Three solutions are combined together in alphabetical order.:
The resulting solution turns yellow, then turns black.
Explanation (including important chemical equations):
This demonstration is a variant of the Landolt or iodine clock reaction.
1. IO3-(aq) + 3 HSO3-(aq) --> I -(aq) + 3 SO42-(aq) + 3 H+(aq)
2. IO3-(aq) + 5 I -(aq) + 6 H+(aq) --> 3 I2 (aq) + 3 H2O (l)
3. I2 (aq) + HSO3-(aq) + H2O (l) --> 2 I -(aq) + SO42-(aq) + 3 H+(aq)
4. I2 (aq) + I -(aq) + starch (aq) --> starch-I3-(aq)
The presence of HgCl2 means that a fifth (and perhaps sixth) reaction can occur.
5. Hg2+(aq) + 2 I -(aq) --> HgI2 (s)
6. HgI2 (s) + 2 I -(aq) --> HgI42-(aq)
The yellow HgI2 precipitate forms as soon as the I - concentration is large enough for the ion product to exceed the solubility product for HgI2. Using the quantities specified above, the HgI2 precipitate does not dissolve. Instead, the yellow suspension of the HgI2 precipitate is masked by the appearance of the deep-blue-black starch-I3- complex when the HSO3- is exhausted.
An alternative form of the demonstration can be prepared by doubling the concentration of HSO3- in solution A. There is now enough HSO3- present initially to consume all of the IO3- ion. The HSO3- is never exhausted and the I - concentration can become high enough to redissolve the HgI2 precipitate. The solution, therefore, turns from clear to yellow and then back to clear again.