Galvanic cells, the Nerst Equation chemistry lab help
1. Cell potential of concentration cell: 0.118
anode half-reaction:
cathode half reaction:
explain why a potential is recorded?
2. Cell potential from complex formation: 0.098
observation of soulution in half-cell: No reaction visible to the eye
explain why the potetnial changes as it does with the addition of the NH3 (aq)
3. Cell potential from precipitate formation: 0.411
observation of soultion in half-life: The clear solution turned a copper/ brown color
explain why the potential changes as it does with the addition of Na2S?
attached is the directions for the section of the lab.
1. Effect of different molar concentrations. Set up the galvanic cell shown in B. Effect of Concentration Figure 32.5, using 1 M CuSO, and 0.001 M CuSo4 solutions. Immerse a polished Changes on Cell Potential copper electrode in each solution. Prepare a salt bridge (Part A.2) to connect the two half-cells. Measure the cell potential. Determine the anode and the cathode. 3 Write an equation for the reaction occurring at each electrode 2. Effect of complex formation. Add 2-5 mL of 6 M NH, to the 0.001 M CuSo, solution until any precipitate redissolves.3 (Caution: Do not inhale NH3,) Observe and record any changes in the half-cell and the cell potentialo 10 3. Effect of precipitate formation. Add 2-5 mL of 0.2 M Na,S to the 0.001 M CuSO, solution now containing the added NH,. What is observed in the half-cell and what happens to the cell potential? Record your observations. o The Nernst Equation
