Show the equation you will use to calculate the volume of 1 M Cu(NO3)2 (aq) need

Question

Show the equation you will use to calculate the volume of 1 M Cu(NO3)2 (aq) needed to prepare a set of solutions that have concentrations in the range of 1 M to 1x10 M in a 10-mL volumetric flask. 1. 2. Write the reduction half-cell eaction for the copper(lI) ion. 3. 4. 5. What is the standard potential for an electrochemical cell that is prepared from a copper half-cell and a zinc half-cell? If the cell potential is negative, which electrode is connected to the anode? Where does the oxidation half-reaction occur, the cathode or the anode?

Explanation / Answer

1) If the solution of 1M Cu(NO3)2 is already prepared the double dilution method can be used to prepare the following concentrations:

0.5M By adding 5ml of 1M Copper nitrate solution and 5 ml of water

0.25M By adding 5ml of 0.5M Copper nitrate solution and 5 ml of water

0.125M By adding 5ml of 0.25M Copper nitrate solution and 5 ml of water

0.0625M By adding 5ml of 0.125M Copper nitrate solution and 5 ml of water

This process can be repeated till the desired range is reached.

Alternately you can use C1V1=C2V2 where C1 = 1 Molar Copper nitrate C2 = New concentration V1=Initial volume of Copper nitrate. V2 volume of Final solution.

2) Reduction Half Cell reaction for Cu(II) ion

Cu2+(aq) + 2e ----------> Cu(s)

Copper moves from oxidation state of +2 in its ion to Cu (Zero) in elemental form. Therefore reduction(by gain of electrons)

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