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November 01, 2025, 01:00:31 pm
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Author Topic: Redox Help  (Read 839 times)  Share 

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Zahta

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Redox Help
« on: October 20, 2012, 07:19:49 pm »
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Can someone please help me  with this question. I know  the second two options cannot work out , because why is it Ag+ that forms a coating on the lead rod because  there is no strong oxidiser reacting with a strong reducer.


Lead rods are placed in solutions of silver nitrate, iron(lI) sulfate and magnesium chloride. In which solutions would you expect to see a coating of another metal form on the lead rod? Explain.


Thankyou to anyone who helps
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nisha

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Re: Redox Help
« Reply #1 on: October 20, 2012, 07:23:59 pm »
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Ag+ is a strong oxidant whilst Pb (s) is a relatively strong reductant. Therefore Ag+ is reduced to Ag(s) -form coating on lead rod- and Pb(s) is oxidised to Pb2+ ions.
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Zahta

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Re: Redox Help
« Reply #2 on: October 20, 2012, 07:58:05 pm »
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okay thanks i just interpreted the pb(s) is a weak reductant since its -0.13, would you call it a weak reductant or you cant?
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aishuwa1995

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Re: Redox Help
« Reply #3 on: October 23, 2012, 02:34:13 pm »
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Quote from: Zahta on October 20, 2012, 07:58:05 pm
okay thanks i just interpreted the pb(s) is a weak reductant since its -0.13, would you call it a weak reductant or you cant?

Pb(s) is a relatively strong reductant if you look at electrochemical series, the things on the right side are ordered in increasing reducing strengths (fluorine ion is the weakest reductant and Li(s) is the strongest). So it's relatively strong because of the position on the electrochemical series, this is how I understand it.
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