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AP EAMCET · Chemistry · Chemical Equilibrium

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

  1. A Shifts the equilibrium towards the formation of \([\mathrm{Fe}(\mathrm{SCN})]^{2+}\)
  2. B Deep red color increases
  3. C Intensity of deep red color decreases
  4. D No change in equilibrium
Verified Solution

Answer & Solution

Correct Answer

(C) Intensity of deep red color decreases

Step-by-step Solution

Detailed explanation

Addition of oxalic acid \(\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4\) causes the oxalate ions \(\mathrm{C}_2 \mathrm{O}_4^{2-}\) to react with \(\mathrm{Fe}^{3+}\) ions and form a complex that decreases the concentration of \(\mathrm{Fe}^{3+}\) ions. Thus, the equilibrium would…