Home
Class 11
CHEMISTRY
The following reaction is at equilibrium...

The following reaction is at equilibrium ,
`underset("Yellow")(Fe_((aq))^(3+))+ underset("Colourless")(SCN_((aq)))rArrunderset("Deep red")([Fe(SNC)]_((aq))^(2+))`
`K_(c)=([Fe(SCN)])/([Fe^(3+)][SCN])`
In the above reaction , colour intensity of red colour can be increased by :-

A

addition of KSCN

B

addition of oxalic acid which reacts with `Fe^(3+)` ions

C

addition of `Hg^(2+)` ions which react with `SCN^(-)` ions

D

red colour intensity cannot be changed.

Text Solution

Verified by Experts

The correct Answer is:
A
Addition of KSCN increases the colour intensity of the solution as it shifts the equilibrium to right. Addition of reagents like oxalic acid or `Hg^(2+)` ions which remove `Fe^(3+)" or SCN"^(-)` ions shift the equilibrium to the left and colour intensity decreases.
Promotional Banner

Topper's Solved these Questions

  • EQUILIBRIUM

    NCERT FINGERTIPS|Exercise Acids, Bases And Salts|9 Videos

  • EQUILIBRIUM

    NCERT FINGERTIPS|Exercise Ionization Of Acids And Bases|19 Videos

  • EQUILIBRIUM

    NCERT FINGERTIPS|Exercise Relation Between Equilibrium Constant Constant, Reaction Quotient And Gibbs Energy|2 Videos

  • ENVIRONMENTAL CHEMISTRY

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

  • HYDROCARBONS

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

Similar Questions

Explore conceptually related problems

Which of the following on addition will cause deep red colour to disappear ? (A) underset("Pale yellow")(Fe^(3+)(aq)) + underset("Colourless")(SCN^(-)(aq))hArr underset("Deep red")([Fe(CNS)^(2)](aq)) I. AgNO_(3)" "II.HgCl_(2)" "III.H_(2)C_(2)O_(4)" " (oxalic acid)

underset("Sulphate")underset("Copper")(CuSO_(4_((aq))))+Fe_((s))rarrunderset("Sulphate")underset("Ferrous")(FeSO_(4_((aq))))+Cu_((S))

Following equilibrium is set up when SCN^(-) ion is added to Fe^(3+) in aqueous solution : underset("Pale yellow")(Fe^(3+))" "+" "underset("Colour less")(SCN^(-))" "hArr" "underset("Deep red")([Fe(SCN)]^(2+)) When silver nitrate is added to the solution, AgSCN gets precipitate. What will happen to the equilibrium?

Influence of pressure, temperature, concentration and addition of inert gas on a reversible chemical reaction in equilibrium can be explained by formulating the expression for equilibrium constant K_(c) or K_(p) for the equilibrium. On the other hand Le Chatelier principle can be theoretically used to explain the effect of P , T or concentration on the physical or chemical equilibrium both. For the reaction: underset(Yellow)(Fe_((aq.))^(3+))+SCN_((aq.))^(-)hArrunderset(Red)([Fe(NCS)]_((aq.))^(2+)) in equilibrium if little more aqueous solution in FeCl_(3) is added, then:

In the following reaction, which is the species being oxidised ? 2Fe_((aq))^(3+)+2I_((aq))^(-) to I_(2(aq))+2Fe_((aq))^(2+)

Complete the following : underset("Blood red colouration")(Fe^(3+) underset("Excess")overset(SCN^(-))to (A) underset("Excess")overset(F^(-)) to (B)) Find the spin magnetic moment of B.

The expression for equilibrium constant, K_(c) for the following reaction is Fe_((aq))^(3+)+3OH_((aq))^(-)hArrFe(OH)_(3(s))