I believe salt is used in the manufacture of paper towel is it not? Removing electrodes to wipe clean with paper towel I accept, but I would not put the paper in the water during production. N.
> From: mrmon...@pstca.com > To: silver-list@eskimo.com > Subject: Re: CS>Keeping the same polarity rods > Date: Sun, 13 May 2012 19:17:49 -0400 > > mgperrault <mgperra...@aol.com> wrote: > > > Why do the grey whiskers get formed on the electrode? > > > If you put a barrier, I used a paper towel, you see they form on > > the paper. Shaking it loose, it fell to the bottom. Adding > > hydrogen peroxide dissolved it to a clear seemingly fine batch. > > >max > > No one has answered your question. Strange. > > The gray whiskers that form on the cathode are pure silver. They are > silver ions from the anode, or positive electrode. They have > accepted an electron from the cathode to become a neutral silver > atom. > > What happens next depends on the current density. At very low > current, such as used in the SilverCell process, the silver forms a > fuzz around the electrode and grows tiny whiskers at the bottom. > > At higher currents, a silver sludge forms at the bottom of the U, > assuming you are using a U-shape electrode. > > At higher currents, such as most cs generators use, the ion density > is high enough for silver hydroxide to form in the thin Nernst > Diffusion layer next to the cathode. > > This forms a soft black/brown deposit on the electrode and sends > some into the dw. It agglomerates later and causes a characteristic > yellow tint to the cs. The color is independent of the size of the > particles. Silver is one of the privileged few metals that react to > light through plasmon absorbance. This resonates with the blue light > and removes it from the spectrum. This leaves red and green, which > combine to form yellow. The yellow portion remains yellow, of > course. This results in the characteristic yellow tint to the cs, > which has been described variously as pale straw, yellow, or gold. > > If you ingest the cs, the silver hydroxide is converted back into > silver ions, which then combine to form silver chloride. You can > read more at > > http://www.mail-archive.com/silver-list@eskimo.com/msg145180.html > > When you add H2O2, the cs may turn clear. It can also turn white, > brilliant yellow, black, and probably other colors. The colors are > probably caused by contamination in the H2O2. > > Silver is a catalyst for H2O2 and causes it to decompose. The > equation is > > 2H2O2 --> 2H2O + O2 > > However, hydrogen peroxide requires a stabilizer to prevent > decomposition. > > The clear color results from the stabilizer in the H2O2 reacting > with the silver hydroxide and producing silver ions. For food grade > H2O2, the stabilizer is phosphoric acid. For pharmaceutical grade, > the stabilizer is a different acid. The bottle should say "Do Not > Ingest", or Poison, or somesuch. They mean it. The additive is > toxic. Don't drink it. > > In the case of food grade H2O2, the phosphoric acid works in > conjunction with the H2O2 to dissolve silver metal into ions. Here's > how it works. Phosphoric acid, H3PO4, has three hydrogen ions > available to ionize. It loses the first one quite readily. (Thanks > to Wilco Oelen of sci.chem for this description) > > H3PO4 <--> H(+) + H2PO4(-) > > This makes hydronium ions (H3O+) available in the solution. If H2O2 > containing H3PO4 is applied to silver metal, we get the following: > > 2Ag + H2O2 + 2H(+) --> 2Ag(+) + 2H2O > > Which is what you want to do. > > There is another side reaction that uses the catalytic reaction to > turn H2O2 into oxygen and water: > > 2H2O2 (plus silver catalyst) --> 2H20 + O2 > > A similar reaction occurs with the silver hydroxide. I can post it > if you wish. > > You cannot measure the conductance of the clear cs with a pwt. The > phosphoric acid will dominate the measurement. But you can use the > Salt Test to verify you still have silver ions in solution. You can > read more on my Yahoo forum at > > http://health.groups.yahoo.com/group/silvercentral/message/560?l=1 > > Does this answer your question? > > I would not use a paper towel or any other kind of paper in cs. The > paper-making process leaves various chemical residues that can > combine with the silver ions and remove them from the solution. > > Recall that you are working with ppm levels of silver ions. Very few > chemistry labs work sith such small concentrations. The > contamination problem is just too expensive to try to to control. > > However, we have no choice. We must learn how to identify and > eliminate as much as possible all the different kinds of > contamination, and keep them from ruining or cs. This is not an easy > problem, especially when most people claim the contamination does > not exist. Please ignore such misinformed opinions. > > Thanks, > > Mike Monett > > > -- > The Silver List is a moderated forum for discussing Colloidal Silver. > Rules and Instructions: http://www.silverlist.org > > Unsubscribe: > <mailto:silver-list-requ...@eskimo.com?subject=unsubscribe> > Archives: > http://www.mail-archive.com/silver-list@eskimo.com/maillist.html > > Off-Topic discussions: <mailto:silver-off-topic-l...@eskimo.com> > List Owner: Mike Devour <mailto:mdev...@eskimo.com> > >
