symboom
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1143
Registered: 11-11-2010
Location: Wrongplanet
Member Is Offline
Mood: Doing science while it is still legal since 2010
|
|
Unique silver compounds
Silver nitrate is combined with these salts
Sodium oxalate
Sodium citrate
Sodium ascorbate
Sodium metabisulfite
Sodium acetate
Sodium chlorocyanurate
Sodium borate....
Sodium silicate...
Magnesium sulfate
Sodium hypochlorite
Insouble yellow silver oxalate
Silver citrate formed is soluble
Sodium ascorbate forms black solid?
Sodium metabisulfite forms pink solid?
Insoluble white silver acetate
Sodium chlorocyanurate forms white percipitate?
silver sulfate slight white cloudyness
silver hypochlorite forms white percipitate
And a little black precipitate
Side notes
Reactions with copper foil
Also if anyone needs copper foil
I extracted mine from a lithium ion battery
Silver acetate
Big chunks spall off the copper foil
Silver citrate
Strongly adheres to the copper foil
Silver sulfate
Percipitate forms on copper surface
[Edited on 9-2-2017 by symboom]
[Edited on 10-2-2017 by symboom]
[Edited on 10-2-2017 by symboom]
|
|
DraconicAcid
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 4299
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
The black solid formed by the reaction with ascorbate is probably metallic silver. Ascorbic acid is a reducing agent.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
|
|
myristicinaldehyde
Hazard to Others
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 166
Registered: 23-4-2016
Location: .͐͌ ͛҉̻̫̰̻̖E̮ͮ̐́̚ ̢̗̅̉ͩ͂̒̌.̯̻̺̯̀̎͂̄ͩ̚
Member Is Offline
Mood: сорок пять
|
|
I would guess the pink precipitate is silver sulfite, which apparently decomposes very readily on exposure to light- this would be the pink color. I
am basing the color source off my experience with silver chloride.
A proof of decomposition causing the pink color rather than the salt itself would be to make some fresh in dim light, then put it in the sun or a UV
light. If it is sulfite, then if you wash it very thoroughly (out of the light) and add a little bit to acid, SO2 should be given off.
If we don't study the mistakes of the future we're doomed to repeat them for the first time.
|
|
Eddygp
National Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 858
Registered: 31-3-2012
Location: University of York, UK
Member Is Offline
Mood: Organometallic
|
|
Why not silver(I) oxide?
there may be bugs in gfind
[ˌɛdidʒiˈpiː] IPA pronunciation for my Username
|
|
woelen
Super Administrator
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 7990
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
Not silver(I) oxide. Silver(I) oxide, when formed in water, is not black, but dirty brown. This is hydrous silver(I) oxide. And indeed, ascorbate is a
sufficiently strong reductor to reduce silver(I) to metallic silver. It also is capable of reducing copper(II) to copper(I).
With bleach you get silver(I) chloride, but you can get a black compound, silver(I) silver(III) oxide, AgAgO2. Hypochlorite is a very strong alkaline
oxidizer and it is capable to oxidize silver to its +3 oxidation state. In this oxidation state it hydrolyses at once and forms a mixed oxidation
state oxide.
|
|
PHILOU Zrealone
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 2893
Registered: 20-5-2002
Location: Brussel
Member Is Offline
Mood: Bis-diazo-dinitro-hydroquinonic
|
|
Quote: Originally posted by woelen ![](images/xpblue/lastpost.gif) | Not silver(I) oxide. Silver(I) oxide, when formed in water, is not black, but dirty brown. This is hydrous silver(I) oxide. And indeed, ascorbate is a
sufficiently strong reductor to reduce silver(I) to metallic silver. It also is capable of reducing copper(II) to copper(I).
With bleach you get silver(I) chloride, but you can get a black compound, silver(I) silver(III) oxide, AgAgO2. Hypochlorite is a very strong alkaline
oxidizer and it is capable to oxidize silver to its +3 oxidation state. In this oxidation state it hydrolyses at once and forms a mixed oxidation
state oxide. |
Silver (III) can be stabilized in water if complexed with ethylenebis(biguanide) and forms then a [ethylenebis(biguanide)silver(III) cation that can
fix nitrate or perchlorate anion
--> [Ag(H2L)]3+ + 3 NO3(-) or 3 ClO4(-)...
Probably energetic ![;)](./images/smilies/wink.gif) ![:)](./images/smilies/smile.gif) ![:cool:](./images/smilies/cool.gif)
PH Z (PHILOU Zrealone)
"Physic is all what never works; Chemistry is all what stinks and explodes!"-"Life that deadly disease, sexually transmitted."(W.Allen)
|
|
symboom
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1143
Registered: 11-11-2010
Location: Wrongplanet
Member Is Offline
Mood: Doing science while it is still legal since 2010
|
|
Quote: Originally posted by woelen ![](images/xpblue/lastpost.gif) |
With bleach you get silver(I) chloride, but you can get a black compound, silver(I) silver(III) oxide, AgAgO2. Hypochlorite is a very strong alkaline
oxidizer and it is capable to oxidize silver to its +3 oxidation state. In this oxidation state it hydrolyses at once and forms a mixed oxidation
state oxide. |
Thank you for the response
I read that silver hypochlorite is formed and disproportionates to silver chloride and silver chlorate
Edit(woelen): Fixed layout issue.
[Edited on 13-2-17 by woelen]
|
|
woelen
Super Administrator
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 7990
Registered: 20-8-2005
Location: Netherlands
Member Is Offline
Mood: interested
|
|
I don't think that silver hypochlorite can form from bleach. Bleach is quite alkaline and under such conditions, you will get silver oxide. Even with
pure hypochlorite, not containing chloride, I expect formation of the black mixed +1/+3 oxide.
|
|
phlogiston
International Hazard
![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif) ![*](images/xpblue/star.gif)
Posts: 1377
Registered: 26-4-2008
Location: Neon Thorium Erbium Lanthanum Neodymium Sulphur
Member Is Offline
Mood: pyrophoric
|
|
Can the slight turbidity observed with sulfate be explained by a slight contamination with lead?
What is the source of your silver nitrate?
When bleach is used to reclaim silver from the gelatine layer of x-ray film, one obtains a white precipitate of (what seems to me to be) silver
chloride. When exposed to sunlight, it converts into a black powder. If kept in the dark, even though bleach is very alkaline it remains white for at
least a few days. Addding concentrated NaOH converts the precipitate to a black powder 'instantly'.
-----
"If a rocket goes up, who cares where it comes down, that's not my concern said Wernher von Braun" - Tom Lehrer
|
|