After reading what Bruce marks says about buffering with baking soda, I
decided to try it.
I dipped a toothpick tip into baking soda to get as little as possible
on it..a clump about the size of 3 or 4 grains of table salt..and swished
that into a pint of distiller water.
I don't remember the exact numbers, but conductivity went way higher than
what I wanted, so I diluted the water down to around 10 uS
I ran a Silverpuppy generator [constant current at 1 ma] on manual till
conductivity when to 30 uS, replicating the average gain on automatic.
It looked like all was going well. Nice and clear, colorless...hummm,
OK, nice stuff.
An hour later the whole thing went dense milky white.
Several hours later, the milkiness was diminishing as a white precipitate
formed and dropped out settling onto the bottom and some gas bubbles formed
on the sides of the jar.
It never completely cleared.
Was that silver carbonate?
Looking around..silver carbonate is light sensitive, has a low
solubility, dissolves in vinegar making silver acetate which is highly
soluble in water.
I set the jar on a North facing window sill. [no 'direct' sunlight]
The white precipitate turned grey.
..added a dollop of white distilled vinegar.
It went clear, colorless, from mega TE to zero TE in a matter of moments.
Everything absolutely dissolved.
I vaguely recall seeing some gas bubbles.
A few days ago, someone confused my phone number with Bruce Marks' number
and called me.
He said he didn't see this happening with a CS Pro generator.
Maybe using unlimited amounts of current does something different, or he
starts and/or stops at a lower conductivity. I dunno..
The only reason baking soda is used to buffer water is to get you to a
certain spot on the 'run away' ramp so you can 'sorta' predict the end
result PPM with a timer. Otherwise, PPM is a total crap shoot.
There is no difference between using CS Pro generator and a set of nine
volt batteries. Constant voltage is constant voltage.
At least Bruce is aware of that problem and offers a way around it, but
I'm pretty sure that using baking soda does affect the end product
regardless of his assertion that it doesn't.
Ode
At 04:48 PM 1/6/2006 -0700, you wrote:
I am curious to see this explored in depth.
I could not see Bruce Marx doing something that was completely unworkable.
Jim
-----Original Message-----
From: Marshall Dudley [mailto:[email protected]]
Sent: Tuesday, December 20, 2005 10:32 AM
To: [email protected]
Subject: CS>Adding bicarb of soda to water for brewing
Adding a very small amount of baking soda to distilled water that has picked
up
some CO2 and formed carbonic acid is very interesting to analyze.
CO2 + H2O -> H2CO3 or carbonic acid
NaHCO3 + H2CO3 -> NaOH + 2CO2 + H2O
If you don't add enough bicarb to neutralize all the carbonic acid, then you
can get this reaction as well:
2NaOH + H2CO3 = Na2CO3 + 2H2O
but then sodium carbonate should react with carbonic acid as well producing:
Na2CO3 + H2CO3 -> 2NaOH + 2CO2
Which puts us right back to the Sodium Hydroxide again.
So unless I am mistaken, the smallest pinch possible of baking soda (or lye)
would neutralize 100% of the carbonic acid in distilled water that has
absorbed
CO2, and as long as no more is added than is necessary to cause all the CO2
to
be released, the effect will be a DECREASE in carbonate, not an increase.
The
sodium hydroxide acts as a catalyst to release CO2. I have put this
question
to some chemists for confirmation and should have a reply shortly.
This appears to be a very interesting topic that needs more study.
Marshall
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