Analytical Chem

The following electrochemical cell can be used to calculate the formation constant Kf for a metal and EDTA. The cell has a voltage of -0.262V. The right half cell contains a metal (M^2+) with a standard reduction potential of -0.236V. Calculate the Kf for the metal EDTA complex.
Citric acid=Pka3=6.396
30mL of 0.010M citric acid
70.0mL of 0.010 NaOH M
30.0mL of 0.010 M M^2+
70.0mL of 0.010M EDTA
alphaY4-=0.81 at pH 11.00
I am trying to get the [H+] concentration first. Then plug into equation... I keep getting 1.99E-07 but not sure if it's right... I think I can do the math from there..

  1. 👍
  2. 👎
  3. 👁
  1. I think the pH comes from the reaction of citric acid with NaOH. That is a buffer.
    ...........H3C + NaOH ==> NaH2C + H2O
    pH = pKa3 + log (base)/(acid)
    pH = 6.396 + log (0.3/0.4) = 6.27 in the anode. Of course the cathode pH is 11.00

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Electrochemistry

    In lab, we did an experiment with electrochemical cells with solutions of ZnSO4, CuSO4, Al2(SO4)3 and MgSO4 and their respective metal electrodes. There are a couple of post-lab questions that I'm not sure about: (1) Summarize

  2. Chemistry

    For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 3.50 M)|Ag(s) write the net cell equation. I presume it is Cu + 2Ag^2+ --> Cu2+ + 2Ag Calculate the following values at 25.0 C using standard potentials as

  3. College Chemistry

    A Galvanic cell consists of Mg electrode in a 1.0 mol L -1 Mg(NO3)2 solution and a Ag electrode in a 1.0 mol L-1 AgNO3 solution. Calculate standard emf for the spontaneous reaction of this electrochemical cell at 25 C, given that

  4. chemistry

    Calculate the standard cell potential for each of the electrochemical cells? 2Ag+(aq)+Pb(s)→2Ag(s)+Pb2+(aq) E∘cell......V? 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s) E∘cell......V? O2(g)+4H+(aq)+2Zn(s)→2H2O(l)+2Zn2+(aq)

  1. AP Chem

    An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminum metal electrode. (a) What is the potential of this cell at 25°C if the aluminum

  2. Chem 1046

    An electrochemical cell is based on these two half-reactions: Ox: Sn(s) → Sn2+(aq, 1.74 M) + 2 e- Red: ClO2(g, 0.120 atm) + e- → ClO2-(aq, 1.44 M) Calculate the cell potential at 25°C E Sn>Sn2+ = -.14 E ClO2 = .95

  3. Chemistry

    Calculate the standard cell potential for each of the following electrochemical cells. Ni^+2(aq)+Mg(s)--->Ni(s)+Mg^+2(aq) I used the e cell values from the back of my book. They are: Ni^+2(aq)+2e--->Ni(s) E^0= -0.23 V

  4. Chemistry/Redox Reactions

    An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminium metal electrode immersed in a solution with [Al3+] = 1.0 M. Sodium hydroxide is

  1. Chemistry

    A nickel-cadmium electrochemical cell functions according to the following reaction: Cd+ Ni2+ → Cu2+ + Ni What is the standard cell potential of a nickel-cadmium electrochemical cell?

  2. chemistry

    Consider an electrochemical cell based on the reaction: 2H+(aq) + Sn(s) = Sn2+(aq) + H2(g). Which of the following actions would NOT change the measured cell potential? lowering the pH in the cathode compartment addition of more

  3. Chemistry

    Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Fe -0.440 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A In the activity, click on the E∘cell and Keq

  4. Chemistry

    What reaction (oxidation or reduction) occurs at an anode of... a) an electrochemical cell OR b) an electrolytic cell

You can view more similar questions or ask a new question.