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Article: Solubility of TTCP and β-TCP by solid titration
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TitleSolubility of TTCP and β-TCP by solid titration
 
AuthorsPan, HB1
Darvell, BW1
 
Keywordsβ-TCP
Solid titration
Solubility
TTCP
 
Issue Date2009
 
PublisherPergamon. The Journal's web site is located at http://www.elsevier.com/locate/archoralbio
 
CitationArchives Of Oral Biology, 2009, v. 54 n. 7, p. 671-677 [How to Cite?]
DOI: http://dx.doi.org/10.1016/j.archoralbio.2008.01.001
 
AbstractObjective: Using solid titration with hydroxyapatite (HAp) and octacalcium phosphate, HAp has been found to be more stable than dicalcium phosphate dihydrate (DCPD) even at lower pH, inconsistent with the widely reported view that DCPD is less soluble than other calcium phosphates below pH 4.2. A check of the behaviour of other calcium phosphates (TTCP; Ca/P: 2.00 and β-TCP; Ca/P: 1.33) is necessary. Methods: Solid titration was used to determine the effective solubility of TTCP and β-TCP in 100 mM KCl solution at 37.0 ± 0.1 °C for pH ∼2.9-9.2 and ∼3-7.4 respectively. The constitution of the precipitate was determined by XRD, particle morphology was observed by SEM and TEM, and the precipitate Ca/P ratio was calculated by EDX. Results: The only identified solid phase at equilibrium was HAp at both pH 3.60 and 4.50; no residual titrant or other phases were detected. A marked change of slope in the curve occurred at pH ∼3.9 for TTCP. Conclusion: HAp was verified to be more stable than other calcium phosphates, especially at lower pH. That DCPD is more stable below pH 4.2 is contradicted. © 2008 Elsevier Ltd. All rights reserved.
 
ISSN0003-9969
2013 Impact Factor: 1.880
2013 SCImago Journal Rankings: 0.677
 
DOIhttp://dx.doi.org/10.1016/j.archoralbio.2008.01.001
 
ISI Accession Number IDWOS:000267480800009
Funding AgencyGrant Number
University of Hong Kong
Funding Information:

This work was done in partial-fulfilment of the requirements for the degree of Ph.D. for Haobo Pan at and supported by the Faculty of Dentistry, The University of Hong Kong. The authors thank P.K.D. Lee and T.D.B. Yuen for technical support; F. Chan for TEM observation; and G-F. Chen for XRD analysis.

 
ReferencesReferences in Scopus
 
DC FieldValue
dc.contributor.authorPan, HB
 
dc.contributor.authorDarvell, BW
 
dc.date.accessioned2011-11-02T03:06:20Z
 
dc.date.available2011-11-02T03:06:20Z
 
dc.date.issued2009
 
dc.description.abstractObjective: Using solid titration with hydroxyapatite (HAp) and octacalcium phosphate, HAp has been found to be more stable than dicalcium phosphate dihydrate (DCPD) even at lower pH, inconsistent with the widely reported view that DCPD is less soluble than other calcium phosphates below pH 4.2. A check of the behaviour of other calcium phosphates (TTCP; Ca/P: 2.00 and β-TCP; Ca/P: 1.33) is necessary. Methods: Solid titration was used to determine the effective solubility of TTCP and β-TCP in 100 mM KCl solution at 37.0 ± 0.1 °C for pH ∼2.9-9.2 and ∼3-7.4 respectively. The constitution of the precipitate was determined by XRD, particle morphology was observed by SEM and TEM, and the precipitate Ca/P ratio was calculated by EDX. Results: The only identified solid phase at equilibrium was HAp at both pH 3.60 and 4.50; no residual titrant or other phases were detected. A marked change of slope in the curve occurred at pH ∼3.9 for TTCP. Conclusion: HAp was verified to be more stable than other calcium phosphates, especially at lower pH. That DCPD is more stable below pH 4.2 is contradicted. © 2008 Elsevier Ltd. All rights reserved.
 
dc.description.naturelink_to_subscribed_fulltext
 
dc.identifier.citationArchives Of Oral Biology, 2009, v. 54 n. 7, p. 671-677 [How to Cite?]
DOI: http://dx.doi.org/10.1016/j.archoralbio.2008.01.001
 
dc.identifier.citeulike5347238
 
dc.identifier.doihttp://dx.doi.org/10.1016/j.archoralbio.2008.01.001
 
dc.identifier.epage677
 
dc.identifier.isiWOS:000267480800009
Funding AgencyGrant Number
University of Hong Kong
Funding Information:

This work was done in partial-fulfilment of the requirements for the degree of Ph.D. for Haobo Pan at and supported by the Faculty of Dentistry, The University of Hong Kong. The authors thank P.K.D. Lee and T.D.B. Yuen for technical support; F. Chan for TEM observation; and G-F. Chen for XRD analysis.

 
dc.identifier.issn0003-9969
2013 Impact Factor: 1.880
2013 SCImago Journal Rankings: 0.677
 
dc.identifier.issue7
 
dc.identifier.pmid19414172
 
dc.identifier.scopuseid_2-s2.0-67349254691
 
dc.identifier.spage671
 
dc.identifier.urihttp://hdl.handle.net/10722/143140
 
dc.identifier.volume54
 
dc.languageeng
 
dc.publisherPergamon. The Journal's web site is located at http://www.elsevier.com/locate/archoralbio
 
dc.publisher.placeUnited Kingdom
 
dc.relation.ispartofArchives of Oral Biology
 
dc.relation.referencesReferences in Scopus
 
dc.subjectβ-TCP
 
dc.subjectSolid titration
 
dc.subjectSolubility
 
dc.subjectTTCP
 
dc.titleSolubility of TTCP and β-TCP by solid titration
 
dc.typeArticle
 
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<description.abstract>Objective: Using solid titration with hydroxyapatite (HAp) and octacalcium phosphate, HAp has been found to be more stable than dicalcium phosphate dihydrate (DCPD) even at lower pH, inconsistent with the widely reported view that DCPD is less soluble than other calcium phosphates below pH 4.2. A check of the behaviour of other calcium phosphates (TTCP; Ca/P: 2.00 and &#946;-TCP; Ca/P: 1.33) is necessary. Methods: Solid titration was used to determine the effective solubility of TTCP and &#946;-TCP in 100 mM KCl solution at 37.0 &#177; 0.1 &#176;C for pH &#8764;2.9-9.2 and &#8764;3-7.4 respectively. The constitution of the precipitate was determined by XRD, particle morphology was observed by SEM and TEM, and the precipitate Ca/P ratio was calculated by EDX. Results: The only identified solid phase at equilibrium was HAp at both pH 3.60 and 4.50; no residual titrant or other phases were detected. A marked change of slope in the curve occurred at pH &#8764;3.9 for TTCP. Conclusion: HAp was verified to be more stable than other calcium phosphates, especially at lower pH. That DCPD is more stable below pH 4.2 is contradicted. &#169; 2008 Elsevier Ltd. All rights reserved.</description.abstract>
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Author Affiliations
  1. The University of Hong Kong