Does temperature affect pH readings. This one has me baffled.

  • We are currently upgrading MFK. thanks! -neo
Where I lived, we also treated with Chloramine.
The raw Lake Michigan water,(pretreatment) entered the treatment plant at a pH of @ 8.4.
After treatment with Chloramine it would drop to 7.6 or at certain seasonal times, 7.2.
I added calcium thiosulfate as a dechloraminator to my tanks during water changes and the pH would rise to @ 8.
Nitrates in the water represent converted ammonia added to turn chlorine, into Chloramine.
In my water treatment facility the ratio was 4 or 5 part chlorine, to 1 part ammonia depending on seasonal organic content to create chloramine.
The treatment ratio where you live may be different, depending on what is needed to make it potable..
Where I lived the ratio showed up as 0.2ppm nitrate on my API test.
Above before dechlorinator, below after.
 
duanes said:
Where I lived, we also treated with Chloramine.
The raw Lake Michigan water,(pretreatment) entered the treatment plant at a pH of @ 8.4.
After treatment with Chloramine it would drop to 7.6 or at certain seasonal times, 7.2.
I added calcium thiosulfate as a dechloraminator to my tanks during water changes and the pH would rise to @ 8.
Nitrates in the water represent converted ammonia added to turn chlorine, into Chloramine.
In my water treatment facility the ratio was 4 or 5 part chlorine, to 1 part ammonia depending on seasonal organic content to create chloramine.
The treatment ratio where you live may be different, depending on what is needed to make it potable..
Where I lived the ratio showed up as 0.2ppm nitrate on my API test.
Above before dechlorinator, below after.
Click to expand...
If I am understanding you correctly you are saying that nitrates are produced from the processing of ammonia to be combined with chlorine to produce chloramine?
 
aussieman57 said:
If I am understanding you correctly you are saying that nitrates are produced from the processing of ammonia to be combined with chlorine to produce chloramine?
Click to expand...
Hi mate
I am fairly new to the site but from what you have explained I believe there are two things happening that are linked to the nitrification process.

Firstly the nitrifying bacteria destroy 7.14 mg of CaC03 alkalinity per 1mg of ammoniam Ion oxidised,. Alkalinity is what keeps the ph stable, but the neutralisation of the hydrogen Ions produced during the nitrification process reduces the CaC03. This in turn is what has reduced your pH (insufficient alkalinity CaC03)

Secondly the nitrification process will all but stall at ph of 6 resulting in the rise in ammonia you are seeing.

The addition of a ph buffer such as sodium Bicarbonate will add much needed alkalinity to maintain the desired ph level.

Hope this makes some sense.
 
  • Like
Reactions: aussieman57
Having a good PH balance is just a myth the fish will be fine whack some water stabilizer in there and cucumber and job done
 
Glen70 said:
Hi mate
I am fairly new to the site but from what you have explained I believe there are two things happening that are linked to the nitrification process.

Firstly the nitrifying bacteria destroy 7.14 mg of CaC03 alkalinity per 1mg of ammoniam Ion oxidised,. Alkalinity is what keeps the ph stable, but the neutralisation of the hydrogen Ions produced during the nitrification process reduces the CaC03. This in turn is what has reduced your pH (insufficient alkalinity CaC03)

Secondly the nitrification process will all but stall at ph of 6 resulting in the rise in ammonia you are seeing.

The addition of a ph buffer such as sodium Bicarbonate will add much needed alkalinity to maintain the desired ph level.

Hope this makes some sense.
Click to expand...
Makes a lot of sense. Did not know this "Firstly the nitrifying bacteria destroy 7.14 mg of CaC03 alkalinity per 1mg of ammoniam Ion oxidised" but that explains a lot of what I am seeing. Appreciate that piece of information. It's a lot easier to deal with a problem when you are aware of the causal effects. Thank you so much.
 
aussieman57 said:
Makes a lot of sense. Did not know this "Firstly the nitrifying bacteria destroy 7.14 mg of CaC03 alkalinity per 1mg of ammoniam Ion oxidised" but that explains a lot of what I am seeing. Appreciate that piece of information. It's a lot easier to deal with a problem when you are aware of the causal effects. Thank you so much.
Click to expand...
No worries, glad I could help ?
 
You must log in or register to reply here.
MonsterFishKeepers.com
Top Bottom