The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal (M) and EDTA. The cell has a potential of −0.266 V. The right half‑cell contains a metal ion (M2+) with a standard reduction potential of −0.236 V.
M2+ + 2e −−⇀↽−M(s) E°=−0.236 V
Citric acid has three pKa values: 3.128, 4.761, and 6.396. Calculate the Kf for the metal–EDTA complex.
Kf=
The electrochemical cell shown can be used to calculate the formation constant (Kf) for a metal...
Page 3 An electrochemical is prepared from a chromium metal electrode in contact solution of 0.500 M chromium (III) nitrate and a standard hydrogen half-cell elect The two half cells are connected by a porous disk or a KCl salt bridge. Standard Reduction Potentials at 298 K Cr+ (aq) + 3e ----> Cr(s) Cr+ (aq) + e ----> Cr2+ (aq) E° = -0.740 V E° = -0.440 V a) Write the reaction for the cell and calculate the standard free...
Prelab Activity: Electrochemical Cells To determine the solubility product of copper(II) carbonate, CuCO3 , a concentration cell as described on pages 71-72 of the lab handout is constructed. The temperature of the Galvanic cell is measured to be 22.5°C, and the cell potential 282 mV (0.282 V). Using this data and Equation 8 in the lab manual, calculate the Ksp for CuCO3 and report your answer with three significant digits. For the Galvanic cell you will construct in PART B,...
need help with the rest of the table EXPERIMENT 10 DETERMINATION OF THE ELECTROCHEMICAL SERIES PURPOSE To determine the standard cell potential values of several electrochemical coll INTRODUCTION The basis for an electrochemical cell is an oxidation reduction Corredor be divided into two half reactions reaction. This reaction can Oxidation half reaction Gloss of electrons) takes place at the anode, which is the positive electrode that the anions migrate to Chence the name anode) Reduction half reaction (gain of electrons)...