Naked Science Forum
Non Life Sciences => Chemistry => Topic started by: Quantum_Vaccuum on 05/10/2007 01:55:33
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How exactly do the ionized hydrogen atoms affect acidity?
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How exactly do the ionized hydrogen atoms affect acidity?
pH = -log10[H+]
where [H+] = concentration hydrogen ions.
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They attach to water molecules to form hydronium ions (H3O+) thats what makes a solution acidic.
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It might also be interesting to note that pH actually means "Power of Hydrogen" so the more Hydrogen ions you have in solution, the more acidic a solution is.
Based on the Lewis Definition, an Acid is a compound which accepts a lone pair of electrons. Hydrogen ions are positively charged and can take up a lone pair of electrons from another compound to form a covalent bond. So the more hydrogen ions you have, the more electron pairs you can accept and the more acidic it becomes.
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It might also be interesting to note that pH actually means "Power of Hydrogen" so the more Hydrogen ions you have in solution, the more acidic a solution is.
Based on the Lewis Definition, an Acid is a compound which accepts a lone pair of electrons. Hydrogen ions are positively charged and can take up a lone pair of electrons from another compound to form a covalent bond. So the more hydrogen ions you have, the more electron pairs you can accept and the more acidic it becomes.
Do you also know at least one example of acid-base reaction not involving H+ ions?
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Aluminium Trichloride (a Lewis acid) with Trimethylamine (a Lewis base) [:)]