The following sections of this BookRags Literature Study Guide is offprint from Gale's For Students Series: Presenting Analysis, Context, and Criticism on Commonly Studied Works: Introduction, Author Biography, Plot Summary, Characters, Themes, Style, Historical Context, Critical Overview, Criticism and Critical Essays, Media Adaptations, Topics for Further Study, Compare & Contrast, What Do I Read Next?, For Further Study, and Sources.
(c)1998-2002; (c)2002 by Gale. Gale is an imprint of The Gale Group, Inc., a division of Thomson Learning, Inc. Gale and Design and Thomson Learning are trademarks used herein under license.
The following sections, if they exist, are offprint from Beacham's Encyclopedia of Popular Fiction: "Social Concerns", "Thematic Overview", "Techniques", "Literary Precedents", "Key Questions", "Related Titles", "Adaptations", "Related Web Sites". (c)1994-2005, by Walton Beacham.
The following sections, if they exist, are offprint from Beacham's Guide to Literature for Young Adults: "About the Author", "Overview", "Setting", "Literary Qualities", "Social Sensitivity", "Topics for Discussion", "Ideas for Reports and Papers". (c)1994-2005, by Walton Beacham.
All other sections in this Literature Study Guide are owned and copyrighted by BookRags, Inc.
The Hydronium ion is an important participant in the chemical reactions that take place in aqueous (water, H20) solutions.
Through a process termed self-ionization, a small number of water molecules in pure water dissociate (separate) in a reversible reaction to form a positively charged H+ ion and a negatively charged OH- ion. In aqueous solution, as one water molecule dissociates, another is nearby to pick up the loose, positively charged, hydrogen proton to form a positively charged Hydronium ion (H3O+).
Water molecules have the ability to attract protons and form Hydronium ions because water is a polar molecule.Oxygen is more electronegative than Hydrogen. As a result, the electrons in each of water's two oxygen-hydrogen bonds to spend more time near the oxygen atom. Because the electrons are not shared equally--and because the bond angles of the water molecule do not cancel out this imbalance--the oxygen atom carries a partial negative charge that can attract positively charged protons donated by other molecules.
In a sample of pure water, the concentration of hydronium ions is equal to 1x10-7 moles per liter (0.0000001 M). The water molecule that lost the hydrogen proton--but that kept the hydrogen electron--becomes a negatively charged hydroxide ion (OH-).
The equilibrium (balance) between hydronium and hydroxide ions that results from self-ionization of water can be disturbed if other substances that can donate protons are put into solution with water. Hydrochloric Acid (HCl), for example, is an important acid found in the human stomach transfers a proton to water to form hydronium ions.
The potential hydronium ion concentration (pH) is equal to the negative logarithm of the hydronium ion concentration: pH=-log [H30+].