Standard hydrogen electrode | Wikipedia audio article
Channel: wikipedia tts
Date: 2019-01-13

This is an audio version of the Wikipedia Article:
https://en.wikipedia.org/wiki/Standard_hydrogen_electrode


00:03:22 1 Relationship between the normal hydrogen electrode (NHE) and the standard hydrogen electrode (SHE)
00:04:41 2 Choice of platinum
00:05:44 3 Interference
00:06:46 4 Isotopic effect
00:07:30 5 Construction
00:08:17 6 See also



Listening is a more natural way of learning, when compared to reading. Written language only began at around 3200 BC, but spoken language has existed long ago.

Learning by listening is a great way to:
- increases imagination and understanding
- improves your listening skills
- improves your own spoken accent
- learn while on the move
- reduce eye strain

Now learn the vast amount of general knowledge available on Wikipedia through audio (audio article). You could even learn subconsciously by playing the audio while you are sleeping! If you are planning to listen a lot, you could try using a bone conduction headphone, or a standard speaker instead of an earphone.

Listen on Google Assistant through Extra Audio:
https://assistant.google.com/services/invoke/uid/0000001a130b3f91
Other Wikipedia audio articles at:
https://www.youtube.com/results?search_query=wikipedia+tts
Upload your own Wikipedia articles through:
https://github.com/nodef/wikipedia-tts
Speaking Rate: 0.9493594012556362
Voice name: en-AU-Wavenet-A


"I cannot teach anybody anything, I can only make them think."
- Socrates


SUMMARY
=======
The  Standard hydrogen electrode (abbreviated SHE), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials. Its absolute electrode potential is estimated to be 4.44 ± 0.02 V at 25 °C, but to form a basis for comparison with all other electrode reactions, hydrogen's standard electrode potential (E0) is declared to be zero volts only at 298K. Potentials of any other electrodes are compared with that of the standard hydrogen electrode at the same temperature.
Hydrogen electrode is based on the redox half cell:

2 H+(aq) + 2 e− → H2(g)This redox reaction occurs at a platinized platinum electrode.
The electrode is dipped in an acidic solution and pure hydrogen gas is bubbled through it. The concentration of both the reduced form and oxidised form is maintained at unity. That implies that the pressure of hydrogen gas is 1 bar (100 kPa) and the activity of hydrogen ions in the solution is unity. The activity of hydrogen ions is their effective concentration, which is equal to the formal concentration times the activity coefficient. These unit-less activity coefficients are close to 1.00 for very dilute water solutions, but usually lower for more concentrated solutions. 
The Nernst equation should be written as:

  
    
      
        E
        =
        
          
            
              R
              T
            
            F
          
        
        ln
        ⁡
        
          
            
              a
              
                
                  
                    H
                    
                      +
                    
                  
                
              
            
            
              
                p
                
                  
                    
                      H
                      
                        2
                      
                    
                  
                
              
              
                /
              
              
                p
                
                  0
                
              
            
          
        
      
    
    {\displaystyle E={RT \over F}\ln {\frac {a_{\mathrm {H^{+}} }}{\sqrt {p_{\mathrm {H_{2}} }/p^{0}}}}}
  
  
    
      
        E
        =
        −
        
          
            
              2.303
              R
              T
            
            F
          
        
        
          p
          H
        
        −
        
          
            
              R
              T
            
            
              2
              F
            
          
        
        ln
        ⁡
        
          
            
              p
              
                
                  
                    H
                    
                      2
                    
                  
                
              
            
            
              p
              
                0
              
            
          
        
      
    
    {\displaystyle E=-{2.303RT \over F}\mathrm {pH} -{RT \over 2F}\ln {\frac {p_{\mathrm {H_{2}} }}{p^{0}}}}
  where:

aH+ is the activity of the hydrogen ions, aH+ = fH+CH+ / C0
pH2 is the partial pressure of the hydrogen gas, in pascals, Pa
R is the universal gas constant
T is the temperature, in kelvins
F is the Faraday constant (the charge per mole of electrons), equal to 9.6485309 × 104 C mol−1
p0 is the standard pressu ...