The first year of our pond the ph was consistently at about 9.0. Second year it was consistently at about 8.5, last year 8.0 and this year 7.5.
I have done nothing to change the ph. Except the fist year adding white vinegar every few days until I got tired of doing it. I thought high ph was better than moving the ph too much so I left it alone.
I wonder if that is typical for a pond as it ages.
Maybe it is the rocks that surround the pond initially leaching more minerals raising the ph and each year as they have been in the pond longer the ph isn't impacted as much by them.
Short answer....
What's been your alkalinity (KH value) through out the period of time and do you primarily use complex calcium carbonate products (i.e., oyster shells, coral, aragonite, etc) ?
Essentially, your pond and critters are maturing. I imagine your fish were smaller and ate less food back during the first year and last year and also I imagine your plants have a better root system now. So, I imagine there is more production and consumption of total ammonia and both of these actions consumes your alkalinity thus allowing your pH to become lower..
Also, as a pond matures, microorganism colonies mature and become more efficient at processing at a lower pH.
My guess is that you are primarily using a complex calcium carbonate product (i.e., oyster shells or coral or aragonite, etc), or some other leaching is involved from stone or other materials, and your pond is reaching its pH equilibrium. pH equilibrium occurs when the consumers and producers come to an "agreement".
This "agreement" will be disrupted once the consumers, such as alkalinity or products releasing alkalinity, starts to decrease, which means either you need to add more complex calcium carbonate products or, depending on how fast your alkalinity falls, then will need to use baking soda (sodium bicarbonate) or gardening potash (potassium carbonate). The potash product is talked about in
post#23 of Raising KH with coral or oyster thread.
Your pond's pH was likely initially high due to the lack of calcium due to leaching, or creation, of carbonates from rocks or other materials/processes into the pond causing the pH to initially be high.
Geeky answer...
KH is one major determining variable in the pH.
In most pond waters, the bicarbonate/carbonate buffer system is most dominant due to most waters encounter various forms of limestone or other complex calcium carbonate rock formations and carbon dioxide. Carbon dioxide is one major actor in creating the bicarbonate/carbonate buffer system since algae, microorganisms, the air, fish, and plants are constantly creating and consuming carbon dioxide.
Three major water equilibria's of the bicarbonate/carbonate buffer system is, as described by the
henderson-hasselbalch equation (
pH = pKa + log([HCO3-]/[H2CO3]) ) and bicarbonate/carbonate equilibriums below:
H2O <-> H+ + OH- ([H+][OH-] = 10^-14)
H2CO3 <-> H+ + HCO3- ([H+][HCO3-]/[H2CO3] = 4.16 x 10^-7)
HCO3- <-> H+ + CO3-- ([H+][CO3--]/[HCO3-] = 4.84 x 10^-11)
HCO3- is bicarbonate and CO32- (CO3--) is carbonate.
KH is the approximate measurement of bicarbonate.
H2CO3 is carbonic acid, which is what is created when carbon dioxide (CO2) dissolves into water (H2O), which is a relatively slow process.
Takes a combination of an acid, such as carbonic acid (H2CO3), and its accompanying salts (HCO3- or CO32-) to create a buffer system.
There is no good measurement of carbonate for hobbyists so we mainly pay attention to pH to try to assume the free calcium concentrations unless a calcium test is used and everyone's required level of free calcium is different. Free calcium neutralizes carbonate (CO32-) by precipitating to create calcium carbonate (CaCO3), which starts to dissolve again when the pH drops below 8.2.
To better understand the bicarbonate/carbonate pH buffer system, then do a google image search for "
freshwater carbonate speciation
bjerrum plot " or
click here for the search results.