Home
Class 12
CHEMISTRY
On the basis of the standard electrode p...

On the basis of the standard electrode potential velues, state whether `Ti^(4+)` species can be used to oxidise Fe(II) to Fe(III).
`Ti^(4+)+e^(-) to Ti^(3+)," "E^(@)=+0.1 V`
`Fe^(3+)+e^(-) to Fe^(2+)," "E^(@)=+0.77 V`

Text Solution

Verified by Experts

Since `Ti^(4+)//Ti^(3+)` has lower `E^(@)` value, then `Fe^(3+)//Fe^(2+)`, it cannot be reduced in comparison to `Fe^(3+)//Fe^(2+)` ions. Hence, `Ti^(4+)` cannot oxidise `Fe^(2+)`to `Fe^(3+)`.
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise IN-TEXT QUESTIONS|15 Videos

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise N.C.E.R.T. EXERCISE|18 Videos

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise ULTIMATE PREPARATORY PACKAGE|12 Videos

  • D-AND -F BLOCK ELEMENTS

    DINESH PUBLICATION|Exercise BRAIN STORMING MULTIPLE CHOICE QUESTIONS (MCQS)|13 Videos

  • ETHERS

    DINESH PUBLICATION|Exercise (MCQs)|8 Videos

Similar Questions

Explore conceptually related problems

(i) On the basis of the standard electrode potential values stated for acid solutions, predict whether Ti^(4+) species may be used to oxidise Fe(II) to Fe(III) {:(Ti^(4+) + e^(-) to Ti^(3+), E^(@) = +0.01V), (Fe^(3+) + e^(-) to Fe^(2+), E^(@)= +0.77V):} (ii) Based on the data arrange Fe^(3+), Mn^(2+) " and " Cr^(2+) in the increasing order of stability of +2 oxidation state. (Give a brief reason) E_(Cr^(3+)//Cr^(2+))^(@) = -0.4V E_(Mn^(3+)//Mn^(2+))^(@) = +1.5V E_(Fe^(3+)//Fe^(2+))^(@) = +0.8V

On the basis of the standard electroe potential values stated for acid solution, predict whether, Ti^(4+) species may be used to oxidise Fe^(II) " to " Fe^(III) . Given. Ti^(4+) +_e^(-) to Ti^(3+),E^(ɵ)=+0.01 V,Fe^(3+)+e^(-) to Fe^(2+),E^(ɵ)=+0.77 V

Given that the standard reduction potentials E ^(0) of Fe^(+2)|Feis 0.26V and Fe ^(+3) |Fe is 0.76V respectively. The E ^(@)of Fe ^(+2)|Fe^(+3) is:

On the basis of the following E^(@) values, the stongest oxidizing agent is [Fe(CN)_(6)]^(4-) rarr [Fe(CN)_(6)]^(3-)+e^(-), E^(@) = -0.35 V Fe^(2+) rarr Fe^(3+)+e^(-), E^(@) = -0.77 V

DINESH PUBLICATION-ELECTROCHEMISTRY-Example
  1. Calculate e.m.f. of the cell containing nickel and copper electrodes. ...

    Text Solution

    |

  2. Write each half cell reaction as well as redox reaction for the follow...

    Text Solution

    |

  3. On the basis of the standard electrode potential velues, state whether...

    Text Solution

    |

  4. Write the cell reaction that occurs when the following half-cells are ...

    Text Solution

    |

  5. A cell is prepared by dipping a copper rod in 1M CuSO(4) solution and...

    Text Solution

    |

  6. Two half cell reactions of an electrons of an cell are given below : ...

    Text Solution

    |

  7. Calculate the emf of the cells formed by the various combinations of t...

    Text Solution

    |

  8. Calculate the reduction potential for the following half cell reaction...

    Text Solution

    |

  9. A zinc rod is dipped in 0.1 M ZnSO(4) solution. The salt is 95% dissoc...

    Text Solution

    |

  10. Represent the cell in which following reaction takes place : Mg(s)+2...

    Text Solution

    |

  11. Calculate E(cell)^(@) for the following reaction at 25^(@)C. A+B^(2...

    Text Solution

    |

  12. Calculate the e.m.f. of the cell in which the following reaction takes...

    Text Solution

    |

  13. The measured e.m.f. at 25^(@)C for the cell reaction , Zn(S)+Cu^(2+)...

    Text Solution

    |

  14. The standard reduction potentials of Cu^(2+)//Cu and Ag^(+)//Ag electr...

    Text Solution

    |

  15. Calculate e.m.f. of the cell, Zn//Zn^(2+)(aq) (0.01 M) ||Cd^(2+) (0.1...

    Text Solution

    |

  16. Calculate the e.m.f. of the cell in which the redox reaction is : Mg...

    Text Solution

    |

  17. Calculate the e.m.f of the cell Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx...

    Text Solution

    |

  18. A voltaic cell is set up at 25^(@)C with following half cells : Ag^(+)...

    Text Solution

    |

  19. A copper-silver cell is set up. The copper ion concentration in it is ...

    Text Solution

    |

  20. Calculate the potential for a half cell reaction containing 0.1 M K(2)...

    Text Solution

    |