In an earlier post I mentioned that PO4 had a small effect on KH. Well, I've been asked for more details, so here goes.
Alkalinity (the buffering capacity) is the sum of all the strong bases in the water, less the amount of H+ (strong acid). For aquaria, it's usually safe to assume that the only significant contributors are bicarbonate, carbonate and phosphate. Specifically, phosphate being trivalent (having 3 negative charges, or the ability to pick up 3 H+'s), phosphate has 3 times the effect on KH as bicarbonate.
Planted aquaria folks, who dose CO2, use the KH-pH-CO2 relationship to estimate our CO2 levels. But the primary assumption of this relationship is alkalinity, which we can measure, is equivalent to KH, which the hobbyist cannot measure.
To that effect, I took a little time to work out how much effect PO4 will have on what we refer to as 'KH'. In other words, how much error will be introduced to the KH term as a result of PO4.
Some numbers to start:
Molar mass of PO4 = 94.97g/mol
Molar mass of OH (alkalinity) = 17.01g/mol
OH is monovalent (one negative charge) sp = 17.01mg/meq.
So, for every ppm of PO4 in our water:
1ppm PO4 = (1mg/L PO4)/ (94.97mg/mmol PO4) = 0.0102mmol/L PO4
Since it's trivalent multiply be 3 = 0.0306meq/L PO4
Converting to units of ppm alkalinity:
(0.0306meq/L)x(17.01mg/meq)=0.54ppm
So each ppm of PO4 adds about 0.5ppm to KH, despite having triple the effect per molecule of bicarbonate. The bottom line is that PO4 has a negligible effect on KH, but sometimes it's nice to prove it to yourself.
Alkalinity (the buffering capacity) is the sum of all the strong bases in the water, less the amount of H+ (strong acid). For aquaria, it's usually safe to assume that the only significant contributors are bicarbonate, carbonate and phosphate. Specifically, phosphate being trivalent (having 3 negative charges, or the ability to pick up 3 H+'s), phosphate has 3 times the effect on KH as bicarbonate.
Planted aquaria folks, who dose CO2, use the KH-pH-CO2 relationship to estimate our CO2 levels. But the primary assumption of this relationship is alkalinity, which we can measure, is equivalent to KH, which the hobbyist cannot measure.
To that effect, I took a little time to work out how much effect PO4 will have on what we refer to as 'KH'. In other words, how much error will be introduced to the KH term as a result of PO4.
Some numbers to start:
Molar mass of PO4 = 94.97g/mol
Molar mass of OH (alkalinity) = 17.01g/mol
OH is monovalent (one negative charge) sp = 17.01mg/meq.
So, for every ppm of PO4 in our water:
1ppm PO4 = (1mg/L PO4)/ (94.97mg/mmol PO4) = 0.0102mmol/L PO4
Since it's trivalent multiply be 3 = 0.0306meq/L PO4
Converting to units of ppm alkalinity:
(0.0306meq/L)x(17.01mg/meq)=0.54ppm
So each ppm of PO4 adds about 0.5ppm to KH, despite having triple the effect per molecule of bicarbonate. The bottom line is that PO4 has a negligible effect on KH, but sometimes it's nice to prove it to yourself.