magnetar68
Member
I was thinking about adding 1 ppm of Ammonia Hydroxide to see if my nitrosyfying bacteria are up to snuff (NH3-->NO2).
The hardware store sells a dilute solution of 10%. I have about 30 gals of water in my 34g tank (the rest of the volume is rock and sand).
For fun, I was trying to calculate how many ml of this 10% solution I need. It has been 20 years since I took chemistry, so I don't think I did this right, but here's what I did:
That seems reasonable, but I have zero confidence I did that correctly.
The hardware store sells a dilute solution of 10%. I have about 30 gals of water in my 34g tank (the rest of the volume is rock and sand).
For fun, I was trying to calculate how many ml of this 10% solution I need. It has been 20 years since I took chemistry, so I don't think I did this right, but here's what I did:
- 30 gals of H2O = 113.56 L of H2O
- There are 1000g/L in water, so this is 113560 grams of water in my 30 gals
- The molecular weight of water is 18.01528 g/mol, so that's 6303.85 mols in 30 gals of water.
- 1 ppm of NH3 would be on million less mols, or 0.0063 mols of NH3
- With a molecular weight of 35.05 g/mol for Ammonia Hydroxide, then I need 0.22095 grams of ammonia hydroxide (0.0063*35.05)
- The density of a fully saturated solution of ammonia hydroxide is 0.88 g/ml (at 59 degrees F), so I would need 0.25 ml of this solution to get 0.221 grams (0.221/0.88).
- With a 10% solution, I would need 10 times that amount, or 2.5 ml (50 metric drops).
That seems reasonable, but I have zero confidence I did that correctly.