As promised, time for some chemistry.
This will cover: pH, Buffering solutions and chelating agents.
NOTE: those of you growing in organic soils can ignore this lesson if so desired. You can not regulate the pH in organic soils better than the plant does, all you can do is muck up the pH and cause problems with your plant.
Back to the lesson
First off we’ll start with pH so those that don’t have a good understanding can follow along with the rest of the lecture
To understand pH, we need to start with pure water H2O or 2 hydrogen atoms and 1 oxygen atom. Even in pure water, not all of the hydrogen is bonded to oxygen, some of the hydrogen is milling about as H+, or single hydrogen atoms with a plus 1 charge, it’s counterpart (or other half is you like) is OH-, or a hydroxyl ion...1 oxygen atom bonded to 1 hydrogen atom and having a charge of -1.
When we measure pH, we are measuring the number of H+ ions (or lack of) in solution. In pure water, even though we have H+, OH- and H2O , the H+ and OH- are in equilibrium so we get a neutral pH of 7.
Now if we add an acid, our pH lowers because we now have an excess of H+ ions in solution. Conversely, if we add a base, our pH rises due to an excess of OH- ions.
Now it may seem simple, but pH is measured on a logarithmic scale meaning that for every point rise or drop we have gained or lost 10x the H+ ions.
Example: pH of 6 has 10X as many H+ ions as a pH 7 and a pH of 5 has 100X more H+ ions than pH7 etc.
So now that we have covered the basics of pH, time for Buffering Solutions.
A buffering solution is a solution with a set pH that resists changes in pH when weak acids or bases are added to it. Because of its nature to resist pH change, and can be tailored to a specific pH, these solutions are widely used in chemical analysis, especially in biological research & testing.
Any of you who have calibrated your pH pen with commercially available solutions has used a buffering agent
Buffering agents need to be chosen carefully because some can also act as chelating agents causing issues with other compounds in your solution. I’ll explain chelating agents later.
Buffering agents work similar to the explanation of water above. It consists of an acid and it’s conjugate base - in water H+ is the acid and OH- is the conjugate base. For this exercise, I am using Citric Acid and it’s conjugate base Sodium Citrate, which also suits our needs for hydroponics due to its ability to be tailored to 6 pH (or a range from 3 to 6.2pH), and it’s common and easy enough to produce.
Now, you may say “what about the sodium, we want to limit how much our plants are exposed to” and you would be right but for explanation purposes we will ignore that issue but address it at a later date when I receive the Citric Acid I ordered and can do a bit of experimenting
I guess maybe I should explain what an acid and it’s conjugate base is
Our acid is Citric Acid => C6H8O7.
Sodium Citrate (our conjugate base) => Na3C6H5O7
Now I have aligned the 2 formulas so you can see the difference, Citric Acid has 8 H atoms and in the base, 3 of these have been replaced by Na (sodium). Once we have our buffering solution set at our chosen pH, here is what takes place when we add more acid/base.
In the case of addition of a base, using NaOH as a base for simplicity, the NaOH dissociates into free Na+ ions and OH- ions. These ions then combine with the Citric acid in solution producing more Sodium Citrate and Water:
NaOH + C6H8O7 => Na3C6H5O7 + 3 (H2O) maintaining our balance
When we add an acid, say HCl (hydrochloric or Muriatic acid), it combines with our conjugate base and we get:
3(HCl) + Na3C6H5O7 => 3(NaCl) + C6H8O7 again maintaining our balance. (salt doesn’t contribute to pH, no H+ ions)
Now in my setup, I will be using Citric acid, but not Sodium Citrate. It’ll take a bit of testing but I think I can solve the sodium issue. As for using Muriatic Acid, I may use it if needed, Chlorine doesn’t concern me as in a well aerated system, it will evaporate quickly.
BTW, anyone wanting to make a pH testing solution for calibrating pens:
mix 17.45g of Citric Acid (powder) with 20.77g of Baking Soda in 800ml distilled water. Once fully dissolved, top up your container to 1 litre and you have a buffered solution with a pH of 6.0
Now that we have covered pH and Buffering solutions, on to Chelating agents. Although they play little to no role in my setup, they are a major concern for salt based hydro systems, and also because some buffering agents can also be chelating agents as well that “could” cause issues for me.
In simplest terms, a chelating agent is a chemical compound that prevents metal ions (Na, Ca, Mg etc) in solution, from interacting with other compounds that may cause them to drop out of solution as precipitate (insoluble forms).
As a example, if you have copper ions in solution and add salt (NaCl), Copper Chloride will form and precipitate as a solid (not soluble in water). By chelating the Copper, we can prevent this from happening.
I have included this also because the Citric Acid I intend to use, can also be a chelating agent.
Well folks, that’s today’s lesson, more to come, you can be sure