Date: Mon, 1 Sep 1997 13:06:11 -0500 From: lasseter@chemvx.chem.tamu.edu (Lasseter Benjamin) To: cp@opus.hpl.hp.com Message-Id: <aabcdefg3322$foo@default> Subject: Re: baking soda, salt
Mark Fisher wrote:
> As you already pointed out, an acid (H+) will react with a base (OH-)
> to form water and a salt, composed of the anion from the acid and the
> cation from the base.
>
> Baking soda, NaHCO3, reacts with any acid to form water, CO2, and a
> sodium salt of the acid, i.e.,
> NaHCO3 + HR --> H20 + CO2 + NaR
>
> where R can be any organic or inorganic anion. For example, if
> vinegar (acetic acid) is used, the end product would be sodium
> acetate, and hydrochloric acid would yield NaCl.
>
> There are a variety of organic acids produced by the
> decomposition/leaching of peat (humic and tannic acid, to name a few),
> so the addition of baking soda would produce quite a mixture of sodium
> salts. This would, of course, raise the pH of the soil, PLUS the
> sodium would displace potassium, an important plant nutrient. This
> would lower the fertility of the soil.
1) A question:
For those who have somewhat higher levels of calcium chloride in
their water, would not the calcium also react with the bicarbonate to LOWER
the pH and form an insoluble salt?
CaCl2 +NaHCO3 --> CaCO3 + NaCl + HCl
I do not remember if this reaction is spontaneous, but I think it is. In
this case, the bicarbonate is an acid, but it leaves behind insoluble
calcium carbonate, which I doubt is altogether healthy.
2) Nonetheless, if Mr Palmer's plants are thriving, there must be
particular conditions which make them thrive. If those conditions involve
the use of baking soda, I should like to learn more about them, as they
could be wise things to replicate. Please, Randy, do post detailed
descriptions of how you grow these baking soda thriving plants.
Benjamin F. Lasseter
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