(C) Addition of oxalic acid $(H_2C_2O_4)$ provides oxalate ions $(C_2O_4^{2-})$,which react with $Fe^{3+}$ ions to form a stable complex $[Fe(C_2O_4)_

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Intensity of deep red color decreases

(C) Addition of oxalic acid $(H_2C_2O_4)$ provides oxalate ions $(C_2O_4^{2-})$,which react with $Fe^{3+}$ ions to form a stable complex $[Fe(C_2O_4)_3]^{3-}$.This reaction significantly decreases the concentration of free $Fe^{3+}$ ions in the solution.According to Le Chatelier's principle,the equilibrium will shift to the left to compensate for the loss of $Fe^{3+}$ ions.As the equilibrium shifts to the left,the concentration of the deep red complex $[Fe(SCN)]^{2+}$ decreases,leading to a decrease in the intensity of the deep red color.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Le-Chaterlier principle and It’s application

Easy

Observe the following equilibrium:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(yellow) (colorless) (deep red)
Addition of aqueous oxalic acid solution to the above equilibrium:

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A
Shifts the equilibrium towards the formation of $[Fe(SCN)]^{2+}$
B
Deep red color increases
C
Intensity of deep red color decreases
D
No change in equilibrium

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6-1.Equilibrium (Chemical Equilibrium)

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Le-Chaterlier principle and It’s application

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Explain the effect of concentration on equilibrium using the following experiment:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(Yellow) (Colourless) (Deep red)

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When an orange solution containing $Cr_{2}O_{7}^{2-}$ ions is treated with an alkali,a yellow solution is formed,and when $H^{+}$ ions are added to the yellow solution,an orange solution is obtained. Explain why this happens.

Medium

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For a reaction $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$,favorable conditions for the reaction to occur in the forward direction are:

MediumAP EAMCET 2022

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In the production of $NO$,the reaction is $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$,$\Delta H = +ve$. This reaction is favored by:

Easy

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In the manufacture of $NH_3$ in Haber's continuous flow process involving the reaction $N_{2(g)} + 3H_{2(g)} \longleftrightarrow 2NH_{3(g)}$,$\Delta H = -22.08 \ kcal$. The favourable conditions are:

MediumAIIMS 2011

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Observe the following equilibrium:$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$(yellow) (colorless) (deep red)Addition of aqueous oxalic acid solution to the above equilibrium:

Similar Questions

Explain the effect of concentration on equilibrium using the following experiment: $Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$ (Yellow) (Colourless) (Deep red)

When an orange solution containing $Cr_{2}O_{7}^{2-}$ ions is treated with an alkali,a yellow solution is formed,and when $H^{+}$ ions are added to the yellow solution,an orange solution is obtained. Explain why this happens.

For a reaction $A_{(g)} + \frac{1}{2} B_{(g)} \rightleftharpoons C_{(g)} + \text{heat}$,favorable conditions for the reaction to occur in the forward direction are:

In the production of $NO$,the reaction is $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$,$\Delta H = +ve$. This reaction is favored by:

In the manufacture of $NH_3$ in Haber's continuous flow process involving the reaction $N_{2(g)} + 3H_{2(g)} \longleftrightarrow 2NH_{3(g)}$,$\Delta H = -22.08 \ kcal$. The favourable conditions are:

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Observe the following equilibrium:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(yellow) (colorless) (deep red)
Addition of aqueous oxalic acid solution to the above equilibrium:

Explain the effect of concentration on equilibrium using the following experiment:
$Fe^{3+}_{(aq)} + SCN^{-}_{(aq)} \rightleftharpoons [Fe(SCN)]^{2+}_{(aq)}$
(Yellow) (Colourless) (Deep red)