Silver Oxide Formation in Electrolysis Experiment

AI Thread Summary
The discussion revolves around an experiment involving the electrolysis of water using silver electrodes. The user observed corrosion at the silver anode, where oxygen is generated, and inquired whether this corrosion results in the formation of silver oxide. Participants emphasize the importance of writing oxidation-reduction equations to understand the process better. The type of electrolyte used in the experiment is also highlighted as a critical factor, with specific mention of sulfuric acid (H2SO4) and caution against using sodium chloride (NaCl) or hydrochloric acid (HCl). The choice of electrolyte can significantly influence the electrolysis outcome and the behavior of the electrodes.
clm321
Messages
58
Reaction score
0
i did an experiment the other day where i split water into hydrogen and oxygen but i used a silver anode and cathode when i turned on the batterie the silver one i think the anode start to corrode( one the one that oxygen forms on) is this making silver oxide when this happens?
 
Chemistry news on Phys.org
Have you tried to write your oxido-reduction equations ?
That would be a good start for you.

It also depends of the electrolyte you used in the solution. H2SO4 ? NaCl ? HCl ? (I hope it's not the two last).
 

Thread 'Solubility of MgSO47H2O in water'

It seems like a simple enough question: what is the solubility of epsom salt in water at 20°C? A graph or table showing how it varies with temperature would be a bonus. But upon searching the internet I have been unable to determine this with confidence. Wikipedia gives the value of 113g/100ml. But other sources disagree and I can't find a definitive source for the information. I even asked chatgpt but it couldn't be sure either. I thought, naively, that this would be easy to look up without...
View full post »

Thread 'Why does having 8 valence electrons make an element inert?'

I was introduced to the Octet Rule recently and make me wonder, why does 8 valence electrons or a full p orbital always make an element inert? What is so special with a full p orbital? Like take Calcium for an example, its outer orbital is filled but its only the s orbital thats filled so its still reactive not so much as the Alkaline metals but still pretty reactive. Can someone explain it to me? Thanks!!
View full post »

Similar threads

Electrolysis: Dark blue oxide from steel?
Replies
6
Views
3K
A question regarding electrolysis
Replies
5
Views
2K
Potassium Chloride Electrolysis
Replies
5
Views
2K
How to clean lead and tin off silver the smart way?
Replies
16
Views
5K
Products of Concentrated Barium Chloride Electrolysis?
Replies
4
Views
3K
Group I/II Metal oxides always basic in aqueous solution -- why?
Replies
3
Views
2K
Removing green copper oxides with Electrolysis, chemicals, etc.
2
Replies
57
Views
10K
Which metal is safest for hair/scalp? Bismuth, silver or zinc oxide?
Replies
9
Views
3K
Electrolysis of NaHCO3 solution with lead electrodes
Replies
2
Views
3K
Isolating CO2 in the electrolysis of Na2CO3 solution
Replies
7
Views
5K

Hot Threads

Recent Insights

Back
Top