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+

For the aqueous Fe(CN)complex K, 1.0x 1035
at 25 °C.
Suppose equal volumes of 0.0030 MFe(NO solution and 0.96 MKCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe
ion.
Round
your answer to 2 signaycant digits.
M
?
Explanation
Check
2019 McGraw-Hill Education. All Rights Reserved.
Terms of Use
Pivacy
X
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For the aqueous Fe(CN)complex K, 1.0x 1035 at 25 °C. Suppose equal volumes of 0.0030 MFe(NO solution and 0.96 MKCN solution are mixed. Calculate the equilibrium molarity of aqueous Fe ion. Round your answer to 2 signaycant digits. M ? Explanation Check 2019 McGraw-Hill Education. All Rights Reserved. Terms of Use Pivacy X

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Expert Answer

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:

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Fe(NO,), +KCN [Fe(CN),]"

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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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[Fe(CN)] [Fe(NO,)[KCN

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