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