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Write the expression for the equilibrium constant, Kc: Kc = [Fe(C2O4)3]^3- / ([Fe^3+] * [C2O4^2-]^3) Show more…
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Kc is 1.67 x 10^-20 at 25°C for the formation of iron (III) oxalate complex ion: Fe^3+(aq) + 3 C2O4^2-(aq) ↔ [Fe(C2O4)3]^3-(aq). If 0.0100 M Fe^3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe^3+ ion at equilibrium?
Madhur L.
Kc is 1.67 × 10^20 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq). If 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?
Sandra L.
What is the concentration of the oxalate ion C2O42- at equilibrium at 25°C if a 0.10 M solution of oxalic acid H2C2O4 was used (Ka1 = 6.5 x 10^-2 and Ka2 = 6.1 x 10^-5)? Question options: a) [C2O42-] = 0.054 M b) [C2O42-] = 0.046 M c) [C2O42-] = 6.1 x 10^-5 M d) [C2O42-] = 2.3 x 10^-11 M The chemical equations are: H2C2O4 → HC2O4- + H+, and HC2O4- → C2O42- + H+. So using ICE tables after the first ionization, [HC2O4-] = [H+] = 0.054 M and [H2C2O4] = 0.046 M. Using a second ICE table, we find: [HC2O4-] = 0.054 M and [C2O42-] = 6.1 x 10^-5 M. Please show conversions of e.g. 6.1 x 10^-5 = [x^2/(0.10)].
Sri K.
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