azmmjadvocates
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got my hands on a RO filter and my issues from a few pages back have cleared up...turns out my well water has a shit ton of calcium in it and adding more (through CalNit) wasn't really working...
hey cool thread! ive a question for you.
What is the best way of preventing oxidation when storing buds? read a few methods and while some of them sound great theyre not practicle for small scale growers with limited bux to do. but still interested to hear your thoughts on it!!
I vacume seal them in my canning jars, you can get a canning jar lid adapter through Cabellas in the vacume sealing section. get both sizes, you will use them both believe me.. Vaccume sealing is a good thing to do in curring as well, get a small thin Digital hydorometer from a cigar shop or online, you can insert it right in with the buds and get a precise reading one when to air them...hey cool thread! ive a question for you.
What is the best way of preventing oxidation when storing buds? read a few methods and while some of them sound great theyre not practicle for small scale growers with limited bux to do. but still interested to hear your thoughts on it!!
Was this the problem with precipitation of salts?
I knew that calcium was to blame--its one of the most likely culprits any time you're getting precipitation (as not many calcium salts are soluble).
My son does that on a regular basis. It can get expensive. ;)Then your intuition is off. I bit off WAAAAAAY more than I can chew this semester. Learned a lesson though.
ok, so here's a good chemistry question:
when determining ppm of P and K in P2O5 and K2O we have to take into consideration the respective molar masses of the elements and thus have conversion factors of .4364 and .83 (close enough) to get out actual ppm of P and K in solution.
for CaNO3 it seems that the calculations people are using don't have a similar factor taken into consideration. this also extends to microelement sources, which leads to my question.
something like Jack's MOST that has 7.5% listed Fe, but in the form of Iron Sulfate. Is 1 g/L still going to be 75 ppm Fe? Or would it be 36.7% of that due to Iron only contributing that much to Iron Sulfate? (I'm not using 75 ppm Fe btw, just easier on the math for the purpose of my point)
By extension, would that mean my N, Ca, and micro numbers are all different that what I thought?
Any thoughts on Jacks Pro Chelated Trace Elements? I'm not sure if I really like the MOST..
When I pour some tap water and watch its pH, over time it becomes more alkaline. Is it due to gasses evaporating or dissolving to or from the nearby air? This happens even after using a carbon filter to remove chlorine.
1ppm = 1 MILLIgram per liter
So if you make up 1M NaCl you really have 1M Na+ and 1M Cl- because you're relying on the number of molecules versus an arbitrary assignment of 0.001g as "1 part per million".
fixed that for ya.
But you got it right here.
:D
so basically, yes..
so dankworth, me, and i imagine many others thinking that we are hitting 120 ppm w/ .774 g/L of CalNit (15.5-0-0-19) are really only achieving the small percentage of Nitrate in the double salt form of calcium nitrate (can't seem to find/too lazy to calculate molar mass of that huge molecule)?
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