Abstract
The apparent failure of the solubility product law to apply to tri-lead phosphate in salt solutions containing excess phosphate is probably due to the formation of intermediate ions whose concentrations and equilibrium relations are not known.
The solubility of tri-lead phosphate in a salt solution of the ionic strength of the blood at pH 7.35 and containing 4 mgm. phosphorus per 100 cc. is quivalent to 3.6 x 10–7 mols of lead per liter. The solubility of lead carbonate in a salt solution of the ionic strength of the blood containing bicarbonate and under carbon dioxide tension comparable to that of the blood is equivalent to 1.0 x 10–6 mols of lead per liter.
Some evidence is added by solubility determinations to support the theory that a double calcium lead phosphate is formed when ionic lead enters the blood stream.
The lactate ion exerts no specific effect upon the solubility of tri-lead phosphate.
Footnotes
- Received December 1, 1928.
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