# 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
Anode:
PH2bar=0.40
30mL of 0.010M citric acid
70.0mL of 0.010 NaOH M
Cathode:
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..
Thanks,

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
I..........0.3...0..........0
add..............0.7...........
C.........-0.3..-0.3.........0.3
E...........0.....0.4........0.3
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. 👎

## 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