001 m as well as with varying tenfold dilutions of

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sulfate with Zn(NO3)2, copper sulfate (1M) with copper sulfate (0.001 M) as well as with varying tenfold dilutions of CuSO4 in deionized water to find out which molar concentration dilution has a similar voltage produced to the unknown copper sulfate. Why we did this: We did this so that we can use our knowledge of the Nernst equation, of the relationship between reduction potential and other variables in an oxidation reaction, and our knowledge of molar concentration to calculate the concentration of the unknown copper. Conclusion: 2
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I used my knowledge of standard potential and redox reactions to find out the potential for each half-cell we calculated, which ended up being not at all similar to our measured voltages from the multimeter, which means that other sources of error (unevenly polished metal pieces, badly calibrated multimeter, badly cleaned glassware, etc) could have caused these inaccuracies. I was also able to conclude that the molar concentration of the unknown CuSO4 solution was a 0.0001M dilution, and I did this by graphing the known(measured) voltages of the various tenfold dilutions of CuSO4. Data: Part 1: Various Galvanic Cells Zn(NO3)2 w/ Zn electrode + CuSO4 w/Cu electrode = 0.615 V MgSO4 w/ Mg electrode + CuSO4 w/Cu electrode = 1.681 V FeSO4 w/ Fe electrode + Zn(NO3)2 w/ Zn electrode = 0.004 V FeSO4 w/ Fe electrode + MgSO4 w/ Mg electrode = 1.064 V Zn(NO3)2 w/ Zn electrode + MgSO4 w/ Mg electrode = 1.088 V CuSO4 w/Cu electrode + FeSO4 w/ Fe electrode = 0.617 V 3
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For the reactions between Zn and Cu, Fe, and Mg the reduction potential was determined for the three half-cells of Cu, Fe, and Mg. The following shows the calculations using the
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