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If an element can exist in several oxida...

If an element can exist in several oxidation states, it is convernient to display the reduction potentials correspondingg to the various half reactions in diagrammatic form, know as latimer diagram the latimer diagram for chlorine in acid solutio is
`CIO_(4)^(-)overset(+1.20V)toCiO_(3)^(-)overset(+1.18V)toHClO_(2)overset(+1.60V)toHClOoverset(1.67V)toCl_(2)overset(1.36V)toCl^(-)` in basic solution.
`ClO_(4)^(-)overset(0.37V)toClO_(3)^(-)overset(0.30V)toClO_(2)^(-)overset(0.68V)toClO^(-)overset(0.42V)toCl_(2)overset(1.36V)toCl^(-)` The standard potentials for two nonadjacent species can also be calculateed by using the concept that `triangleG^(@)` as an additive property but potential is not an additive property and `triangleG^(@)=-nFx^(0)`. if a given oxidation stateis a stronger oxidising agent than the next higher oxidation state, disproportionation can occur. The reverse of disproportionation is called comproportionation. The relative stabilities of the oxidation state can also be understood by drawing a graph of `triangleG^(@)//F` against oxidation state, known as frost diagram, choosing the stability of zero oxidation state arbitrarily as zero. The most stable oxidation state of a species lies lowest in the diagram, disproportionation is spontaneous if the species lies above a straight line joining its two product species.
Q. Which of the following couple have same value of potential at `pH=0` and `pH=14?`

A

`(ClO_(4)^(-))/(ClO_(3)^(-))`

B

`(ClO_(2)^(-))/(Cl_(2))`

C

`(ClO_(2)^(-))/(Cl_(2))`

D

`(Cl_(2))/(Cl^(-))`

Text Solution

Verified by Experts

The correct Answer is:
D
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Similar Questions

Explore conceptually related problems

If an element can exist in several oxidation states, it is convernient to display the reduction potentials correspondingg to the various half reactions in diagrammatic form, know as latimer diagram the latimer diagram for chlorine in acid solutio is CIO_(4)^(-)overset(+1.20V)toCiO_(3)^(-)overset(+1.18V)toHClO_(2)overset(+1.60V)toHClOoverset(1.67V)toCl_(2)overset(1.36V)toCl^(-) in basic solution. ClO_(4)^(-)overset(0.37V)toClO_(3)^(-)overset(0.30V)toClO_(2)^(-)overset(0.68V)toClO^(-)overset(0.42V)toCl_(2)overset(1.36V)toCl^(-) The standard potentials for two nonadjacent species can also be calculateed by using the concept that triangleG^(@) as an additive property but potential is not an additive property and triangleG^(@)=-nFx^(0) . if a given oxidation stateis a stronger oxidising agent than the next higher oxidation state, disproportionation can occur. The reverse of disproportionation is called comproportionation. The relative stabilities of the oxidation state can also be understood by drawing a graph of triangleG^(@)//F against oxidation state, known as frost diagram, choosing the stability of zero oxidation state arbitrarily as zero. The most stable oxidation state of a species lies lowest in the diagram, disproportionation is spontaneous if the species lies above a straight line joining its two product species. Q. For a hypothetical element, the frost diagram is shown in figure.? which of the following oxidation state is least stable?

If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-) In basic solution is : ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-) . The standard potentials for two nonadjacent species can also be calculated by using the concept that DeltaG^(@) is an additive property but using potential is not an assitive property and DeltaG^(@)=-nFx^(0), If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of DeltaG^(@)//F against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. For a hypothetical element, the Frost diagram is shown in figure Which of the following oxidation state is least stable ?

Knowledge Check

  • If an element can exist in several oxidation states, it is convernient to display the reduction potentials correspondingg to the various half reactions in diagrammatic form, know as latimer diagram the latimer diagram for chlorine in acid solutio is CIO_(4)^(-)overset(+1.20V)toCiO_(3)^(-)overset(+1.18V)toHClO_(2)overset(+1.60V)toHClOoverset(1.67V)toCl_(2)overset(1.36V)toCl^(-) in basic solution. ClO_(4)^(-)overset(0.37V)toClO_(3)^(-)overset(0.30V)toClO_(2)^(-)overset(0.68V)toClO^(-)overset(0.42V)toCl_(2)overset(1.36V)toCl^(-) The standard potentials for two nonadjacent species can also be calculateed by using the concept that triangleG^(@) as an additive property but potential is not an additive property and triangleG^(@)=-nFx^(0) . if a given oxidation stateis a stronger oxidising agent than the next higher oxidation state, disproportionation can occur. The reverse of disproportionation is called comproportionation. The relative stabilities of the oxidation state can also be understood by drawing a graph of triangleG^(@)//F against oxidation state, known as frost diagram, choosing the stability of zero oxidation state arbitrarily as zero. The most stable oxidation state of a species lies lowest in the diagram, disproportionation is spontaneous if the species lies above a straight line joining its two product species. Q. Which of the following statement is correct?

    A
    `Cl_(2)` undergoes disproportionation into `Cl^(-)` and `ClO^(-)` both at `pH=0` and `pH=14`.
    B
    `Cl_(2)` undergoes disproportionation into `Cl^(-)` at `pH=14` but not at `pH=0`
    C
    `Cl_(2)` undergoes disproportionation into `Cl^(-)` and `ClO^(-)` at `pH=0` but not at `pH=14`
    D
    none of these

  • If an element can exist in several oxidation states, it is convernient to display the reduction potentials correspondingg to the various half reactions in diagrammatic form, know as latimer diagram the latimer diagram for chlorine in acid solutio is CIO_(4)^(-)overset(+1.20V)toCiO_(3)^(-)overset(+1.18V)toHClO_(2)overset(+1.60V)toHClOoverset(1.67V)toCl_(2)overset(1.36V)toCl^(-) in basic solution. ClO_(4)^(-)overset(0.37V)toClO_(3)^(-)overset(0.30V)toClO_(2)^(-)overset(0.68V)toClO^(-)overset(0.42V)toCl_(2)overset(1.36V)toCl^(-) The standard potentials for two nonadjacent species can also be calculateed by using the concept that triangleG^(@) as an additive property but potential is not an additive property and triangleG^(@)=-nFx^(0) . if a given oxidation stateis a stronger oxidising agent than the next higher oxidation state, disproportionation can occur. The reverse of disproportionation is called comproportionation. The relative stabilities of the oxidation state can also be understood by drawing a graph of triangleG^(@)//F against oxidation state, known as frost diagram, choosing the stability of zero oxidation state arbitrarily as zero. The most stable oxidation state of a species lies lowest in the diagram, disproportionation is spontaneous if the species lies above a straight line joining its two product species. Q. Which of the following statement is correct?

    A
    `A^(+1)` undergoes disproportionation into A and `A^(2+)`
    B
    `A^(2+)` undergoes disproportionation in A and `A^(3+)`
    C
    A undergoes comporportionation in `A^(+1)` and `A^(-1)`
    D
    All of the above.

  • If an element can exist in several oxidation states, it is convernient to display the reduction potentials correspondingg to the various half reactions in diagrammatic form, know as latimer diagram the latimer diagram for chlorine in acid solutio is CIO_(4)^(-)overset(+1.20V)toCiO_(3)^(-)overset(+1.18V)toHClO_(2)overset(+1.60V)toHClOoverset(1.67V)toCl_(2)overset(1.36V)toCl^(-) in basic solution. ClO_(4)^(-)overset(0.37V)toClO_(3)^(-)overset(0.30V)toClO_(2)^(-)overset(0.68V)toClO^(-)overset(0.42V)toCl_(2)overset(1.36V)toCl^(-) The standard potentials for two nonadjacent species can also be calculateed by using the concept that triangleG^(@) as an additive property but potential is not an additive property and triangleG^(@)=-nFx^(0) . if a given oxidation stateis a stronger oxidising agent than the next higher oxidation state, disproportionation can occur. The reverse of disproportionation is called comproportionation. The relative stabilities of the oxidation state can also be understood by drawing a graph of triangleG^(@)//F against oxidation state, known as frost diagram, choosing the stability of zero oxidation state arbitrarily as zero. The most stable oxidation state of a species lies lowest in the diagram, disproportionation is spontaneous if the species lies above a straight line joining its two product species. Q. What is the potential couple (ClO^(-))/(Cl^(-)) at pH=14 ?

    A
    `1.78V`
    B
    `-0.94V`
    C
    `0.89V`
    D
    `-0.89V`

    • Similar Questions

    Explore conceptually related problems

    If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-) In basic solution is : ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-) . The standard potentials for two nonadjacent species can also be calculated by using the concept that DeltaG^(@) is an additive property but using potential is not an assitive property and DeltaG^(@)=-nFx^(0), If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of DeltaG^(@)//F against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. What is the potential of couple (ClO^(-))/(Cl^(-)) at pH = 14 14?

    If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-) In basic solution is : ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-) . The standard potentials for two nonadjacent species can also be calculated by using the concept that DeltaG^(@) is an additive property but using potential is not an assitive property and DeltaG^(@)=-nFx^(0), If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of DeltaG^(@)//F against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. Which of the following couple have same value of potential at pH = 0 and pH = 14?

    If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-) In basic solution is : ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-) . The standard potentials for two nonadjacent species can also be calculated by using the concept that DeltaG^(@) is an additive property but using potential is not an assitive property and DeltaG^(@)=-nFx^(0), If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of DeltaG^(@)//F against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. Which of the following statement s correct ?

    If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-) In basic solution is : ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-) . The standard potentials for two nonadjacent species can also be calculated by using the concept that DeltaG^(@) is an additive property but using potential is not an assitive property and DeltaG^(@)=-nFx^(0), If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of DeltaG^(@)//F against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. Which of the following statement is correct according to above question ?

    Latimer diagram for Cu in an acidic solution is: Cu^(+2) overset(+0.15V)toCu^(+) overset(+0.50)toCu,

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