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Related Concept Videos

Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
Ions as Acids and Bases02:54

Ions as Acids and Bases

Salts with Acidic Ions
Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Aqueous salt solutions, therefore, may be acidic, basic, or neutral, depending on the relative acid-base strengths of the salt’s constituent ions. For example, dissolving the ammonium chloride in water results in its dissociation, as described by the equation:
Determining the pH of Salt Solutions04:08

Determining the pH of Salt Solutions

The pH of a salt solution is determined by its component anions and cations. Salts that contain pH-neutral anions and the hydronium ion-producing cations form a solution with a pH less than 7. For example, in ammonium nitrate (NH4NO3) solution, NO3− ions do not react with water whereas NH4+ ions produce the hydronium ions resulting in the acidic solution. In contrast, salts that contain pH-neutral cations and the hydroxide ion-producing anions form a solution with a pH greater than 7. For...
Polyprotic Acids03:38

Polyprotic Acids

Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
Common Ion Effect03:24

Common Ion Effect

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 Châtelier’s principle. Consider the dissolution of silver iodide:
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...

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Related Experiment Video

Updated: Jul 7, 2026

Simultaneous pH Measurement in Endocytic and Cytosolic Compartments in Living Cells using Confocal Microscopy
09:46

Simultaneous pH Measurement in Endocytic and Cytosolic Compartments in Living Cells using Confocal Microscopy

Published on: April 28, 2014

Stable five- and six-coordinated silicate anions in aqueous solution.

S D Kinrade1, J W Del Nin, A S Schach

  • 1Department of Chemistry, Lakehead University, 955 Oliver Road, Thunder Bay, Ontario, Canada P7B 5E1. Stephen.Kinrade@lakeheadu.ca

Science (New York, N.Y.)
|September 8, 1999
PubMed
Summary

Simple sugar-like molecules form stable silicon complexes in water. This finding supports theories on silicon

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Area of Science:

  • Chemistry
  • Biochemistry
  • Geology

Background:

  • Silicon is essential in biological systems and geological processes.
  • Understanding silicon's aqueous chemistry is crucial for various scientific fields.

Purpose of the Study:

  • To investigate the formation of stable silicon-polyol complexes in aqueous solutions.
  • To explore the role of polyols in silicon coordination chemistry.

Main Methods:

  • Aqueous silicate solutions were reacted with aliphatic polyols.
  • Characterization of the resulting polyolate complexes was performed.

Main Results:

  • High concentrations of stable five- or six-coordinated silicon-polyolate complexes were formed.
  • Polyols with at least four hydroxyl groups, including a threo configuration, effectively coordinated with silicon.
  • Coordination occurred via hydroxyl oxygens adjacent to the threo pair.

Conclusions:

  • Aliphatic polyols readily form hypervalent silicon complexes in water.
  • These complexes likely play a key role in biological silicon transport and mineral diagenesis.