Part C: These dilutions were used 1 M Cu2+ 0.01M Cu2+ 0.0001M Cu2+ 0.000001M Cu2

Question

Part C: These dilutions were used

1 M Cu2+

0.01M Cu2+

0.0001M Cu2+

0.000001M Cu2+

A battery is made from electrochemical cells. Referencing the Nernst equation, explain why a battery dies. The Vernier pH sensor functions by measuring a voltage between two electrochemical cells and converts that to a pH value. One half of the electrochemical cell is the solution that is being tested, and the other half is a Ag-AgCl cell within the sensor. With this information, explain why the pH measurement of deionized water may not make sense. Activity is often more appropriate to use when making electrochemical measurements than concentration. Activity is the "effective concentration" of a species or ion relative to a standard (1 M) and accounts for non-ideal behavior of a solution. How does the notion of activity influence your conclusion in Part C How could we account for this in our experiment You likely observed bubbles when you placed Mg metal in the Mg2+solution. Explain the formation of the bubbles and write the two half reactions involved.

Explanation / Answer

there are four questions..

i am explaining two questions only first and last

1) The battery dies as the concentration of the electrolyte is used up.resulting in no further oxidation and reduction of the electrolyte .

4) The Mg gets oxidised and the H2 gas is released which appears as bubbles.

The reactions are as follows :

Anode : Mg ------> Mg+2 + 2e

Cathode : 2 H2O + 2e ----> H2   + 2OH-

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