<p>Electrolysis of a dilute solution of sodium chloride results in the cathode product: Hydrogen.</p>
<p>How does hydrogen come into play... I was really surprised when I saw the answer. Can someone explain this? Thanks</p>
<p>I’m pretty sure that electrolysis involves water, which is where the Hydrogen shows up.</p>
<p>^ That is factually correct, but has nothing to do with the process. It is because Hydrogen has a greater Electrode potential meaning it is more easily reduced than Sodium. Shaqtus you’ve been asking a lot of easy explainable questions from the book that have these answers, are you sure you are ready for the test? o.o</p>
<p>Thanks for the encouragement bud! /sarcasm</p>
<p>(LEO goes GER)
(RED CAT/ AN OX)</p>
<p>We are dealing with reduction (Cathode), so what is reduced in the solution:</p>
<p>Na+ Cl- H2O… which element is the easiest to be reduced (is willing to gain an electron): The answer is obviously Na or H. </p>
<p>They would have to give you reduction potentials, but for the record:</p>
<p>Eo(H)>Eo(Na)</p>
<p>The ions that will be present are Na+, Cl-, H+ and OH-. Since the cathode is negatively charged , it will attract the positively charged ions which are Na+ and H+. At an electrode, either oxidation or reduction occurs and since it is the cathode we are talking about, there will be reduction. And the ion which is discharged is always the one with a higher reduction potential. Since H+ has the higher potential, it will be discharged to At the electrode, the one that will be discharged is the one with a higher reduction potential, it will be reduced to form hydrogen gas.
2H+ + 2e –> H2(g)</p>