Acid-Base Reactions Medical Presentation

Acid Base Reactions PowerPoint Presentation

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Published on : Apr 27, 2018 | Views : 1909 | Downloads : 13

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Acid-Base Reactions
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Johannes N. Brønsted (1879–1947) and Thomas M. Lowry (1874–1936) defined that
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There are three types of Acid-Base Reactions Strong Acid with Strong Base Weak Acid with Strong Base or Strong Acid with Weak Base
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Acid-Base Titration A titration involves delivery (from a buret) of a measured volume of a solution of known concentration (the titrant) into a solution containing the substance being analyzed (the analyte). The point in the titration where enough titrant has been added to react exactly with the analyte is called the equivalence point or the stoichiometric point. This point is often marked by an indicator, a substance added at the beginning of the titration that changes color at (or very near) the equivalence point. The point where the indicator actually changes color is called the endpoint of the titration.
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Example
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Redox Reactions
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In this reaction, solid sodium, which contains neutral sodium atoms, reacts with chlorine gas, which contains diatomic Cl2 molecules, to form the ionic solid NaCl, which contains Na and Cl ions.
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Oxidation States (Numbers) We define the oxidation states (or oxidation numbers) of the atoms in a covalent compound as the imaginary charges the atoms would have if the shared electrons were divided equally between identical atoms bonded to each other or, for different atoms, were all assigned to the atom in each bond that has the greater attraction for electrons. Of course, for ionic compounds containing monatomic ions, the oxidation states of the ions are equal to the ion charges. Note that it can be fraction as in Fe3O4.
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The Characteristics of Oxidation–Reduction Reactions With this background, we can now define some important terms. Oxidation is an increase in oxidation state (a loss of electrons). Reduction is a decrease in oxidation state (a gain of electrons). Thus in the reaction Methane is oxidized and Oxygen is reduced. In addition, O2 is called the oxidizing agent (electron acceptor), and CH4 is called the reducing agent (electron donor).
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Balancing Oxidation–Reduction Equations
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For Example
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Example
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