Why is a large excess of Fe3+ added when preparing the standard solution. But you not add a large excess of Fe3+ when preparing the equilibrium solution.
Fe^3+ + SCN^- = FeSCN^2+
Fe3+ + SCN- = FeSCN2+
A very large concentration of Fe3+ is added to a small concentration (known) of SCN- ( shown as [SCN-]0) to prepare standard solution. The [Fe3+] taken is 100 times than [Fe3+] in the equilibrium mixtures.
To understand the reason of that, we have to consider Le
Chatelier's principle, this high concentration of reactant forces
the reaction far toward formation of products, using up nearly 100%
of the
[SCN-]0.
Thus in the prepared standard solution [FeSCN2+] is assumed to be equal to [SCN-]0 initially taken.
Why is a large excess of Fe3+ added when preparing the standard solution. But you not...
Why is a large excess of Fe3+ added when preparing the standard solution. Why do you not add a large excess of Fe3+ when preparing the equilibrium solution. Fe^3+ + SCN^- = FeSCN^2+?
Fe3+ (aq) + ow does the equilibrium shift a) if you add more Fe* SCN (aq) = FeSCN2+ (aq) Fes b) if you remove SCN c) if you remove FeSCN+2 d) if you add more Fe" and you remove FeSCN2 e) if you remove Fe" and you remove FeSCN+2
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