Chemistry

posted by .

One half-cell of a concentration cell consists of a silver wire dipping into a 1.00 M solution of Ag+. The second half-cell consists of a silver electrode in a solution containing an unknown concentration of Ag+. The measured cell potential was determined as 226 mV at 25°C. Calculate the molarity of Ag+ in the unknown solution to 3 significant figures.

  • Chemistry -

    E(cell) = Eo - (0.0592/n)log(dil/concd)
    Does the problem give any information to tell you which way the electrons are flowing? If not, all I know to do is to work it both ways; i.e., we don't know which solution is the more concentrated. IF we assume the concn of the unknown is less (often the known is made to be 1 M), then we substitute
    0.226 for Ecell
    0 for Eo
    n = 1
    dil we will call the x value
    concd we will call 1 M.
    Solve for x, the concn of the more dilute solution.
    NOW, you can reverse that if you wish and recalculate x (making dil 1 and concd in the denominator x) and solve for x and compare the two values. One will be realistic and the other will not. Post your work if you get stuck. I worked the problem and my answer was 1.52 x 10^-4 M (the other value was 6750 M if I reversed the numbers). Clearly, 6750 M is not very realistic. Check my thinking. Check my arithmetic.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact …
  2. Chemistry

    A chemist wishes to determine the concentration of CrO4-2 ions electrochemically. A cell is constructed consisting of saturated calomel electrode (SCE) and a silver wire coated with Ag2CrO4. The SCE is composed of mercury in contact …
  3. chemisry

    Two half cells in a galvanic cell consist of one iron electroide in a solution of iron sulphate and a silver electrode in a silver nitrate solution a) Assume that the cell is operating as a galvanic cell. State the oxidation half reaction, …
  4. Chemistry

    Little confusing!! I need help PLZ!!! Two half cells in a galvanic cell consist of one iron (Fe(s)) electrode in a solution of iron (II) sulphate (FeSO4(aq)) and a silver (Ag(s)) electrode in a silver nitrate solution. a. Assume the …
  5. chemistry

    Consider the cell: (Pt) H2/H+ || (Pt) H+/H2. In the anode half-cell, hydrogen gas at 1.0 atm is bubbled over a platinum electrode dipping into a solution that has a pH of 7.0. The other half-cell is identical to the first except that …
  6. CHEMISTRY

    The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction …
  7. Chemistry

    Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in …
  8. chem 2

    Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in …
  9. Chemistry

    What will be the potential of a cell constructed of a standard hydrogen electrode as one half-cell and a silver wire coated with AgBr dipping into 0.13 M HBr as the other half-cell?
  10. Chemistry

    One half-cell in a voltaic cell is constructed from a silver wire electrode in a .25 M solution of AgNO3 . The other half-cell consists of a zinc electrode in a .001 M solution of Zn(NO3)2. Calculate the cell potential I have no idea …

More Similar Questions