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An experiment with Le Chatelier's Principle resulted in this equation: Fe3+ + SCN- <=> Fe(SCN)2+ First...

An experiment with Le Chatelier's Principle resulted in this equation: Fe3+ + SCN- <=> Fe(SCN)2+

First off, should the first reactant be Fe2+ or Fe3+? Our TA said Fe2+, but I'm not sure why it's not Fe3+ since we were adding Fe3+ to observe changes in equilibrium. (The lab manual specifies that Fe(SCN)2+ in a product.)

Second, it was obvious that adding Fe3+ and SCN- shifted the equilibrium to the right toward products. However, addition of NaH2PO4 shifted the equilibrium left, back toward the reactants. What is it about NaH2PO4 that caused this to happen?

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queen_honey_blossom answered 1 year ago
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