# For the aqueous Fe(CN)complex K, 1.0x 1035at 25 °C.Suppose equal volumes of 0.0030 MFe(NO solution and 0.96 MKCN solution are mixed. Calculate the equilibrium molarity of aqueous Feion.Roundyour answer to 2 signaycant digits.M?ExplanationCheck2019 McGraw-Hill Education. All Rights Reserved.Terms of UsePivacyX

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Asked Dec 2, 2019
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Calculate the equilibrium molarity of aqueous Fe^2+

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Step 1

Given information:

Concentration of Fe(NO3)2 = 0.0030 M

Concentration of KCN = 0.96 M

Kf = 1.0×1035

Step 2

The reaction between Fe(NO3)2 and KCN to given [Fe(CN)6]4- is represented as follows:

Step 3

The equilibrium constant can be written as the ratio of concentration of products to the concentration of reactants raised to some power of their stoichiometric coefficient. It is represented by Keq or Kc.

The concentration of ...

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