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**To**:**Aquatic-Plants at actwin_com****Subject**:**Re: Can someone check my math?****From**:**"Jamie Johnson" <jjohnson at davisfloyd_com>**- Date: Wed, 11 Apr 2001 08:49:33 -0400

Jerry Leong wrote: > Aaron Ivers wrote: > Subject: Can someone check my math? > Is it acceptable to assume that 1 mL of this stuff then > represents (1000 mg x 97% x 30%) or 291 mg of PO4? > > Also sounds good. >>Concentrated Phosphoric Acid is much denser than water (approx. 1.8(?) for a 97% concentration) - a 30% sol. is approx. 1.2. This means that unless your calculations include the differences due to the specific gravity and if you are using a volume measurement (ml), you'll be adding approximately 20% more phosphate than you think you're adding.<< Since you're using volumes, density _doesn't_ matter. 1 ml still contains a solution with a concentration of 291,000 mg per liter PO4. 1 ml is 1/1000 of a liter, or: 1 ml x 291,000 ug/ml = 291,000 ug = 291 mg. If you didn't have a way of measuring volume, you could theoretically weigh out the solution to get 1 ml total volume, which would be ~1.2 g, based on a density of 1.2 g/cc. 1.2 g / (1.2 g/cc) = 1 cc = 1ml. Jamie <"\\\>< Aquatic plants, water chemistry, and cichlids Greenwood, SC http://www.ais-gwd.com/~jjirons

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