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Related Concept Videos

Titration of Polyprotic Base with a Strong Acid01:18

Titration of Polyprotic Base with a Strong Acid

The titration of a polyprotic base such as sodium carbonate with a strong acid such as hydrochloric acid results in two equivalence points on the titration curve. At the first equivalence point, the carbonate ions in the base are completely converted to bicarbonate ions. The second equivalence point corresponds to the complete conversion of bicarbonate ions to carbonic acid, which dissociates into carbon dioxide and water. The region before the first equivalence point corresponds to the...
Titration of Polyprotic Acids with a Strong Base01:23

Titration of Polyprotic Acids with a Strong Base

Titration of a polyprotic acid, which contains multiple ionizable protons, involves distinct dissociation steps, each with its own dissociation constant (Ka). Each successive Ka is weaker than the previous one. In the titration of a polyprotic acid like sulfurous acid with a strong base such as sodium hydroxide, the base first neutralizes the initial ionizable proton, forming an intermediate species (e.g., hydrogen sulfite ions). This step's titration curve resembles that of a weak monoprotic...
Titration of a Polyprotic Acid02:08

Titration of a Polyprotic Acid

A polyprotic acid contains more than one ionizable hydrogen and undergoes a stepwise ionization process. If the acid dissociation constants of the ionizable protons differ sufficiently from each other, then the titration curve for such polyprotic acid generates a distinct equivalence point for each of its ionizable hydrogens. Therefore, titration of a diprotic acid results in the formation of two equivalence points, whereas the titration of a triprotic acid results in the formation of three...
Factors Affecting Solubility04:01

Factors Affecting Solubility

Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
Titration Calculations: Strong Acid - Strong Base02:28

Titration Calculations: Strong Acid - Strong Base

Calculating pH for Titration Solutions: Strong Acid/Strong Base
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH. The pH at different volumes of added base solution can be calculated as follows:
(a) Titrant volume = 0 mL. The solution pH is due to the acid ionization of HCl. Because this is a strong acid, the ionization is complete and the hydronium ion molarity is 0.100 M. The pH of the solution is then:
Titration Calculations: Weak Acid - Strong Base03:55

Titration Calculations: Weak Acid - Strong Base

Calculating pH for Titration Solutions: Weak Acid/Strong Base
For the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH, the reaction can be represented as:

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Related Experiment Video

Updated: Jun 22, 2026

Optimized Procedure for Determining the Adsorption of Phosphonates onto Granular Ferric Hydroxide using a Miniaturized Phosphorus Determination Method
08:21

Optimized Procedure for Determining the Adsorption of Phosphonates onto Granular Ferric Hydroxide using a Miniaturized Phosphorus Determination Method

Published on: May 18, 2018

Solid titration of octacalcium phosphate.

H-B Pan1, B W Darvell

  • 1Dental Materials Science, Faculty of Dentistry, University of Hong Kong, Hong Kong, SAR, China.

Caries Research
|June 27, 2009
PubMed
Summary
This summary is machine-generated.

Octacalcium phosphate (OCP) solubility is complex, often forming more stable hydroxyapatite (HAp). This study used solid titration to investigate OCP, finding HAp is the more stable phase in bone and dental applications.

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Optimized Procedure for Determining the Adsorption of Phosphonates onto Granular Ferric Hydroxide using a Miniaturized Phosphorus Determination Method
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Area of Science:

  • Biomineralization
  • Materials Science
  • Physical Chemistry

Background:

  • Octacalcium phosphate (OCP) is crucial for dental enamel and bone formation.
  • Hydroxyapatite (HAp) is the stable end-phase in bone, but OCP's solubility product (pK(sp)) is debated.
  • HAp formation may obscure OCP's true solubility due to its greater stability.

Purpose of the Study:

  • To accurately determine the solubility product (pK(sp)) of octacalcium phosphate (OCP).
  • To investigate the phase transformations and stability of OCP under varying pH conditions.
  • To clarify the role of OCP as a precursor in calcium phosphate precipitation.

Main Methods:

  • Solid titration was employed to study OCP in 100 mM KCl at 37°C.
  • X-ray diffraction (XRD) and selected-electron area diffraction (SEAD) identified precipitate phases.
  • High-resolution field emission scanning electron microscopy (FEG-SEM), transmission electron microscopy (TEM), and energy-dispersive X-ray analysis (EDX) characterized morphology and elemental composition.

Main Results:

  • The titration curve spanned pH 3.4–7.4.
  • Hydroxyapatite (HAp) was the primary precipitate at pH 3.6 and 4.5, with no residual OCP detected.
  • Dicalcium phosphate dihydrate (DCPD) formed at pH 3.6 upon further OCP addition, suggesting metastable formation.
  • HAp seeding confirmed HAp as the more stable phase, preventing OCP solubility isotherm determination in the studied pH range.

Conclusions:

  • Hydroxyapatite (HAp) is confirmed as the most stable calcium phosphate phase under the experimental conditions.
  • The study casts doubt on dicalcium phosphate dihydrate (DCPD) being the most stable phase below pH 4.2.
  • Metastable DCPD formation is possible via Ostwald's rule, dependent on supersaturation and nucleation.