Home
Class 12
CHEMISTRY
The potential of the cell Cu, Cu^(2+) (...

The potential of the cell `Cu, Cu^(2+) (0.1M)"//"HCl (xM), Cl_(2), Pt`is 1.07 V. If the standard potential of copper and chlorine electrodes are 10.34 V and 1.36 V, calculate the concentration of HCI.

Text Solution

Verified by Experts

The correct Answer is:
`0.01 M`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise EXERCISE - 4.1.4|4 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise EXERCISE - 4.1.5|3 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise EXERCISE - 4.1.2|13 Videos

  • DILUTE SOLUTIONS

    AAKASH SERIES|Exercise EXERCISE - 1.2|55 Videos

  • ELEMENTS OF D - BLOCK

    AAKASH SERIES|Exercise EXERCISE - 5.2|33 Videos

Similar Questions

Explore conceptually related problems

The EMF of the cell Ni//Ni^(2+)(0.01)// // Cl^(-)(0.01M)//Cl_(2) , pt is -----V if the SRP of nickel and chlorine electrodes are -0.25V and +1.36V respectively

Standard oxidation potential of iron electrode is + 0.44 V. Calculate the potential of Fe, FeSO_4(0.1 M) at 25^@C .

The cell reaction of a cell is Mg(s) + Cu^(2+)(aq) to Cu(s) + Mg^(2+)(aq) If the standard reduction potentials of magensium and copper are -0.33 and +2.38 V respectively, the emf of the cell is

If the standard electrode protential of Cu^(2+)// Cu electrode is 0.34 V , what is the electrode potential at 0.01 M concentration of Cu^(2+) ? (T = 298^(@) K)

At 25^@C potential of the cell, Pt, H_2(g), HCl (aq)"//"AgCl(s), Ag(s) is 0.22 V. If E^@ of silver electrode is 0.8 V , calculate the solubility of AgCI in water .

For the cell , Hg,Hg_2 Cl_2//Cl (0.1M)//Cl^(-)(0.01M)//Cl_2, Pt E_("cell")^@ is 1.10V , Hence , E_("cell") is

For the cell reaction, Mg_((s))+Cu_((aq))^(2+) rarr Cu_((s)) +g^(2+)(aq.) the standard reduction potentials of Mg and Cu are -2.37 V and 0.34 V respectively. The e.m.f. of the cell is

Consider the following four electrode : A = Cu^(2+) (0.0001 M)// Cu(S) B= Cu^(2+) (0.1M)//Cu(s) C = Cu^(2+) (0.01 M )//Cu(s) D) = Cu^(2+) (0.001 M )// Cu(s) If the standard reduction potential of Cu^(+2)// Cu is + 0.34 V , the reduction potential ( in volts ) of the above electrodes follow the order

Aluminium displaces hydrogen from acids, but copper does not. A galvanic cell prepared by combining Cu//Cu^(2+) and Al//Al^(3+) has an emf of 2.0 V at 298K. If the potential of copper electrode is +0.34V, that of Aluminium electrode is

E.m.f. of the cell Zn|Zn^(2+)(1)||Cu^(2+)(1M)|Cu is 1.1 volt. If the standard reduction potential of Zn^(2+)|Zn is -0.78 volt, what is the oxidation potential of Cu|Cu^(2+) ?

AAKASH SERIES-ELECTROCHEMISTRY -EXERCISE - 4.1.3
  1. How is electrical energy generated by performing a chemical reaction ?

    Text Solution

    |

  2. Describe the construction and working of Daniell cell.

    Text Solution

    |

  3. What is single electrode potential? How is it dependent on various fac...

    Text Solution

    |

  4. Write the Nernst equation for a metal electrode and for a non-metal el...

    Text Solution

    |

  5. Describe the constitution of standard hydrogen electrode.

    Text Solution

    |

  6. What is electrochemical series ? Write different applications of the s...

    Text Solution

    |

  7. How are the cells systemically represented ? Given examples.

    Text Solution

    |

  8. E(Ag^(+),Ag)^(0) = 0.8 V . Calculate the single electrode potential in...

    Text Solution

    |

  9. E^@ values of Zn^(2+), Zn and Cu^(2+), Cu are respectively -0.76 V a...

    Text Solution

    |

  10. The potential of the cell Cu, Cu^(2+) (0.1M)"//"HCl (xM), Cl(2), Ptis...

    Text Solution

    |

  11. Represent the cell in which the following reaction takes place Mg(s)...

    Text Solution

    |

  12. E^(@) value of Co^(2+), Co, Al^(3+) , Al , Ag^(+), Ag and Ba^(2+), Ba ...

    Text Solution

    |

  13. E^@ for Mg to 2e^(-) + Mg^(2+) is + 2.37 V and for Cu to 2e^(-) + Cu ...

    Text Solution

    |

  14. Standard reduction potential of I(3)^(-), I^(-) and Fe^(3+), Fe^(2+) ...

    Text Solution

    |

  15. Two students use of the same stock solutions of zinc sulphate and a so...

    Text Solution

    |

  16. Calculate the equilibrium constant of the reaction : Cu((s))+2Ag((aq)...

    Text Solution

    |

  17. The standard emf of Deniell cell is 1.1 V. Calculate the standard Gibb...

    Text Solution

    |