RelativeResourceManager(13) - equations one must know the...

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13 of 17 Example 6 . 40 g of soil is extracted with 120 ml of NH 4 OAc. 5 ml of extract is diluted to 120 ml with water. You know that this soil contains 0.16 meq Na/100 g soil. What concentrations of Na (in ppm) do you expect to find upon analysis of the final dilution? Answer: 0.51 ppm Na+ VI. OXIDATION-REDUCTION REACTIONS Oxidation is the process which results in the loss of one or more electrons by atoms. Fe 2+ - e -  Fe 3+ or Fe 2+  Fe 3+ + e - Reduction is the process which results in the gain of one or more electrons by atoms. Fe 3+ + e -  Fe 2+ An oxidizing agent is one that gains electrons and is reduced to a lower valence state. 2(+l) 2(+6) 7(-2) 2(+3) K 2 Cr 2 O 7 + 6e -  2 Cr 3+ + . .. A reducing agent is one that loses electrons and is oxidized to a higher valence state. +2 -2 +3 Fe SO 4 - e -  Fe 3+ + . .. To determine the equivalent weight of oxidizing or reducing agents or to balance redox
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Unformatted text preview: equations one must know the oxidation number of the element. The oxidation number of an element is a number which, applied to that element in a particular compound, indicates the amount of oxidation or reduction which is required to convert one atom of the free state to that of the compound. The following rules apply to the determination of oxidation numbers. 1. The oxidation number of the free or uncombined element is 0. 2. The oxidation number of the hydrogen ion has a value of +1. 3. The oxidation number of oxide oxygen is -2. 4. The oxidation number of a metal in a compound is usually positive. 5. The oxidation number of a radical or ion is equal to the electrical charge. 6. The oxidation number of a compound is always zero and is determined by the sum of the individual atoms each multiplied by the number of atoms of the element in the molecule....
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