- #1
Latsabb
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It has been a bit since I took chemistry, but I have been wondering something, and can't seem to remember. Let's say that I have the following:
Fe3+ + SCN- <-> FeSCN2+
How can I calculate the point where Fe3+ concentrations become effectively zero? That would say, if I know that I have 1M Fe3+ in a solution, and I plan to add SCN- in large amounts to put pressure on the left side, forcing the reaction to the right, how can I calculate the concentration of SCN- needed to make the Fe3+ run out?
Thanks in advance.
Fe3+ + SCN- <-> FeSCN2+
How can I calculate the point where Fe3+ concentrations become effectively zero? That would say, if I know that I have 1M Fe3+ in a solution, and I plan to add SCN- in large amounts to put pressure on the left side, forcing the reaction to the right, how can I calculate the concentration of SCN- needed to make the Fe3+ run out?
Thanks in advance.