To determine the concentration of copper ions in a copper sulfate solution using an electrochemical cell and a standard hydrogen electrode SHE , follow these steps:1. Prepare the electrochemical cell: a. Set up a half-cell containing the copper sulfate solution with a copper electrode Cu immersed in it. b. Set up another half-cell containing a standard hydrogen electrode SHE with a platinum electrode Pt immersed in a 1.0 M HCl solution. c. Connect the two half-cells with a salt bridge to allow the flow of ions between them. d. Connect the copper electrode and the platinum electrode to a voltmeter to measure the cell potential.2. Measure the cell voltage: a. Turn on the voltmeter and record the cell potential E_cell in volts.3. Calculate the standard reduction potentials: a. The standard reduction potential for the SHE is 0 V by definition. b. The standard reduction potential for the Cu2+/Cu half-cell is +0.34 V.4. Calculate the cell potential using the Nernst equation: a. The Nernst equation is E_cell = E_cell - RT/nF * ln Q , where E_cell is the standard cell potential, R is the gas constant 8.314 J/molK , T is the temperature in Kelvin assume 298 K if not given , n is the number of electrons transferred in the redox reaction 2 for Cu2+/Cu , F is the Faraday constant 96485 C/mol , and Q is the reaction quotient. b. Calculate E_cell by subtracting the standard reduction potential of the SHE from that of the Cu2+/Cu half-cell: E_cell = 0.34 V - 0 V = 0.34 V. c. Rearrange the Nernst equation to solve for Q: Q = exp E_cell - E_cell * nF / RT . d. Plug in the values and calculate Q.5. Determine the concentration of Cu2+ ions: a. The reaction quotient Q = [Cu2+] / [H+]^2, where [Cu2+] is the concentration of copper ions and [H+] is the concentration of hydrogen ions 1.0 M in the SHE half-cell . b. Rearrange the equation to solve for [Cu2+]: [Cu2+] = Q * [H+]^2. c. Plug in the values and calculate the concentration of Cu2+ ions in the copper sulfate solution.By following these steps, you can determine the concentration of copper ions in a copper sulfate solution using an electrochemical cell and a standard hydrogen electrode.