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Water: A Bronsted-Lowry Acid and Base

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 Bases

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 Solutions

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 Acids

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 Effect

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 Acid

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

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Aniones de silicato estables de cinco y seis coordenadas en solución acuosa.

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

Resumen

Las moléculas simples similares al azúcar forman complejos estables de silicio en el agua. Este hallazgo apoya las teorías sobre el silicio.

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Área de la Ciencia:

Química Química es la química.
La bioquímica es la bioquímica.
Geología Geología Geología.

Sus antecedentes:

El silicio es esencial en los sistemas biológicos y los procesos geológicos.
Comprender la química acuosa del silicio es crucial para varios campos científicos.

Objetivo del estudio:

Para investigar la formación de complejos estables de silicio-poliol en soluciones acuosas.
Explorar el papel de los polioles en la química de coordinación del silicio.

Principales métodos:

Las soluciones acuosas de silicato fueron reaccionadas con polioles alifáticos.
Se realizó la caracterización de los complejos de poliolato resultantes.

Principales resultados:

Se formaron altas concentraciones de complejos estables de cinco o seis poliolatos de silicio coordinados.
Poliolos con al menos cuatro grupos hidroxilo, incluida una configuración treo, efectivamente coordinados con silicio.
La coordinación se produjo a través de oxígenos hidroxilo adyacentes a la pareja threo.

Conclusiones:

Los polioles alifáticos forman fácilmente complejos de silicio hipervalentes en el agua.
Es probable que estos complejos jueguen un papel clave en el transporte biológico de silicio y la diagenesis mineral.