Using the following ICE table, What would be the concentration of ferric iron ionsFe³+) and thiocyanate ions (NCS¯) after equilibrium?Fe³+ + NCS <=> {FeSCN}2+SubstanceInitialChangeEquilibriumFe3+(aq)7.14 x 10-4 M-XNCS™(aq)1.07 x 10-3-X↑{FeSCN}2+(aq)0+X4.32 x 10-4 0SubstanceInitialChangeEquilibriumFe3+(aq)7.14 x 10-4 M-XNCS™(aq)1.07 x 10-3-X{FeSCN}2+(aq)0+X4.32 x 10-4The equilibrium constant (Qeq) for this reaction not under standard stateconditions will have a value of

Answered: Using the following ICE table, What…

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Using the following ICE table, What would be the concentration of ferric iron ions
Fe³+) and thiocyanate ions (NCS¯) after equilibrium?
Fe³+ + NCS <=> {FeSCN}2+
Substan
ce
Initial
Change
Equilibri
um
Fe3+
(aq)
7.14 x 10-4 M
-X
NCS™
(aq)
1.07 x 10-3
-X
↑
{FeSCN}2+
(aq)
0
+X
4.32 x 10-4

0
Substan
ce
Initial
Change
Equilibri
um
Fe3+
(aq)
7.14 x 10-4 M
-X
NCS™
(aq)
1.07 x 10-3
-X
{FeSCN}2+
(aq)
0
+X
4.32 x 10-4
The equilibrium constant (Qeq) for this reaction not under standard state
conditions will have a value of

Expert Solution

Step 1

Introduction

According to the question,

$T h e i n i t i a l c o n c e n t r a t i o n o f t h e F e^{2 +} i s g i v e n = 7.14 \times 10^{- 4} M T h e i n i t i a l c o n c e n t r a t i o n o f t h e N C S^{-} i s g i v e n b y = 1.07 \times 10^{- 3} M T h e f i n a l c o n c e n t r a t i o n o f t h e {F e S C N}^{2 +} = 4.32 \times 10^{- 4} M$

Find- The concentration of the ions at equilibrium and equilibrium constant.

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