I posted this on the NCRC site and was directed to as for Norm, since he was crowned the king of chemistry.
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I was wondering if anyone here has mixed their own supplements. Specifically, I want to make a potassium nitrate (KNO3) solution. It has a molar mass of 101.1032 g/mol with a composition of:
K: 38.672%
N: 13.854%
O: 47.474%
This leads me to think that every gram of KNO3 will have 61.328% NO3 and 38.672% K. To make numbers easier, let's say 60% NO3 and 40% K. The potassium is an upside for my carbon dosed tank, but I want to dose NO3.
Here is where I am confused:
I have a 66G NWV tank, which is equivalent to ~250L. If I want to raise NO3 by 1 PPM, then I take 250,000 mL / 1,000,000 mL to get 0.25 mL of a compound. Does this sound right?
Now to get 0.25mL of a NO3, I need to get 0.25mL/0.60 g of KNO3 into solution which is .4167 g of KNO3. Does this sound right?
I can measure out .4167 g of KNO3 and dump it in the tank or I can dissolve .4167 g of KNO3 into 1mL of water. I can dose that 1mL of water into the tank for the same effect. If I dissolve 41.67 g of KNO3 into 100mL of H2O, I now have a stock of solution I can dose into the tank at 1PPM of NO3 per mL. If I dissolve the same 41.67 g of KNO3 into 500mL of H2O, I can dose 5mL of the solution to increase the tanks NO3 concentration by 1PPM. Does this sound right?
By the same token I will increasing the K of the tank by 0.67 PPM, but this is negligible.
Any advice or pointers are appreciated.
--snip--
--snip--
I was wondering if anyone here has mixed their own supplements. Specifically, I want to make a potassium nitrate (KNO3) solution. It has a molar mass of 101.1032 g/mol with a composition of:
K: 38.672%
N: 13.854%
O: 47.474%
This leads me to think that every gram of KNO3 will have 61.328% NO3 and 38.672% K. To make numbers easier, let's say 60% NO3 and 40% K. The potassium is an upside for my carbon dosed tank, but I want to dose NO3.
Here is where I am confused:
I have a 66G NWV tank, which is equivalent to ~250L. If I want to raise NO3 by 1 PPM, then I take 250,000 mL / 1,000,000 mL to get 0.25 mL of a compound. Does this sound right?
Now to get 0.25mL of a NO3, I need to get 0.25mL/0.60 g of KNO3 into solution which is .4167 g of KNO3. Does this sound right?
I can measure out .4167 g of KNO3 and dump it in the tank or I can dissolve .4167 g of KNO3 into 1mL of water. I can dose that 1mL of water into the tank for the same effect. If I dissolve 41.67 g of KNO3 into 100mL of H2O, I now have a stock of solution I can dose into the tank at 1PPM of NO3 per mL. If I dissolve the same 41.67 g of KNO3 into 500mL of H2O, I can dose 5mL of the solution to increase the tanks NO3 concentration by 1PPM. Does this sound right?
By the same token I will increasing the K of the tank by 0.67 PPM, but this is negligible.
Any advice or pointers are appreciated.
--snip--