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Dissolution Kinetics of Iron-, Manganese-, and Copper-Containing Synthetic Hydroxyapatites

^a Dep. of Soil and Crop Sciences, Texas A&M Univ., College Station, TX 77843
^b NASA Johnson Space Center, Houston, TX 77058
^c SETI Institute, NASA Ames Research Center, Moffett Field, CA 94035

View larger version (34K): [in a new window]   Fig. 1. Calcium release rates versus time for pure-SHA, Fe12-SHA, Mn11-SHA, and Cu12-SHA treated with deionized water, citric acid, and DTPA.

View larger version (35K): [in a new window]   Fig. 2. Phosphorus release rates versus time for pure-SHA, Fe12-SHA, Mn11-SHA, and Cu12-SHA treated with deionized water, citric acid, and DTPA.

View larger version (19K): [in a new window]   Fig. 3. Calcium/P molar ratio release versus time of Mn11-synthetic hydroxyapatite (SHA) treated with deionized (DI) water, DTPA, and citric acid. Line represents solid Ca/P SHA molar ratio as calculated from Table 2. Error bars are standard deviation of the mean.

View larger version (22K): [in a new window]   Fig. 4. Infrared spectra of pure-, Fe12-, Mn11-, and Cu12-synthetic hydroxyapatite (SHA) materials exposed to deionized water and 0.1 mM citric acid. Arrows indicate the vibrational modes of calcium citrate that occurred between 1573 and 1579 cm–1.

View larger version (22K): [in a new window]   Fig. 5. Manganese, Cu, and Fe release rates from Fe12-, Mn11-, and Cu12-synthetic hydroxyapatite (SHA) in deionized (DI) water and citric acid.

View larger version (17K): [in a new window]   Fig. 6. Manganese, Cu, and Fe release rates from Fe12-, Mn11-, and Cu12-synthetic hydroxyapatite (SHA) in DTPA.