The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO 3 ) 2 are mixed with 1.0 L of 1.0 M Na 2 C 2 O 4 .The oxalate ion,C 2 O 4 ,acts as a ligand to form a complex ion with the Mn 2+ ion with a coordination number of two. Mn 2+ + C 2 O 4 2 - MnC 2 O 4 K 1 = 7.9 $\times$ 10 3 [Mn(C 2 O 4 ) 2 ] 2 - MnC 2 O 4 + C 2 O 4 2 - K 2 = 1.26 $\times$ 10 - 2 -Find the equilibrium concentration of the [Mn(C₂O₄)₂]²^- ion. A)9.2 $\times$10^-⁵ M B)0.01 M C)2.5 $\times$10^-⁸ M D)1.3 $\times$ 10^-⁴ M E)6.7 $\times$ 10^-³ M

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The question appears to be asking for the equilibrium concentration of a complex ion, but the options provided are in a format that includes encoded characters, making it difficult to interpret the values correctly. However, based on the format, option E seems to be chosen as the correct answer, likely due to a specific calculation or understanding of equilibrium chemistry principles relevant to the context of the question. Without the actual context or values, a precise explanation cannot be provided, but typically, equilibrium concentrations are determined through calculations involving equilibrium constants and initial concentrations of reactants and products.

The Following Questions Refer to the Following System: 500 ×\times× 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 =

The Following Questions Refer to the Following System: 500 $\times$ 10³
[Mn(C₂O₄)₂]²^-
MnC₂O₄+ C₂O₄²^-
K₂ =