Oxidation-reduction equations basic solutions

Balancing oxidation-reduction equations for reactions occurring in aqueous acidic solutions is usually fairly straightforward since we can use H20 to balance O, and then H+ to balance H. In basic solution,... 

Balance the oxidation-reduction equation for the oxidation of Zn(s) by NaN03(aq) to produce Na2Zn (OH)4 and NH3(aq) in basic aqueous solution. 

The general procedure is to balance the equations for the half-reactions separately and then to add them to obtain the overall balanced equation. The half-reaction method for balancing oxidation-reduction equations differs slightly depending on whether the reaction takes place in acidic or basic solution. 

Balancing Oxidation-Reduction Equations Occurring in Basic Solution by the Half-Reaction Method... 

Although the preceding skeleton equation is not complete, it does give the essential information about the oxidation-reduction reaction. Moreover, given the skeleton equation, you can complete and balance the equation using the half-reaction method. Let us see how to do that. We first look at balancing oxidation-reduction equations in acidic solution. To balance such equations in basic solution requires additional steps. 

To balance an oxidation—reduction equation in basic solution, you begin by balancing the equation as if it were a reaction in acidic solution. Then, you add the following steps. ... 

Additional Steps for Balancing Oxidation-Reduction Equations in Basic Solution... 

Balancing equations in acidic and basic solutions by the half-reaction method Given the skeleton equation for an oxidation-reduction equation, complete and balance it. (EXAMPLES 20.1,20.2)... 

Balance the following oxidation—reduction equations. The reactions occur in basic solution. 

Oxidation-reduction equations are now balanced using half-reactions in acidic or basic solutions. 

Balance each of the following skeletal equations by using oxidation and reduction half-reactions. All the reactions take place in basic solution. Identify the oxidizing agent and reducing agent in each reaction. 

Write partial equations for the oxidation and the reduction. Then (1) Balance charges by adding in acid solutions or OH in basic solutions. (2) Balance the number of O s by adding H O s to one side. (3) Balance the number of H s by adding H s to one side. The number added is the number of equivalents of oxidant or reductant. 

Civilization depends on the protection of metals, for most of them are unstable in normal environments unless they are protected by some kind of oxide film. The basic idea about the theory of corrosion is that the metal gets involved in a kind of local fuel cell in which it consumes itself. The partner to most of this self-dissolution is the deposition of hydrogen (favored in acid solutions) or the reduction of oxygen (favored in alkaline). Corrosion is measured in many ways, but the quick way in the laboratory is to move the potential a little bit away ( 5 mV) from the corrosion potential in both anodic and cathodic directions and measure the corresponding current. A simple equation takes the data from this type of measurement and produces the corrosion rate. 

Most aqueous reaction equations can be balanced by trial and error. Oxidation-reduction reactions require a more systematic approach to balancing equations using either an acidic or basic solution. 

In basic aqueous solution, coordinated carbon monoxide can act as a reducing agent with carbonate being the oxidation product for the case of a mononuclear compound undergoing a two-electron reduction (equation 39). 

Oxidation-reduction reactions can occur in basic as well as in acidic solutions. The half-reaction method for balancing equations is slightly different in such cases. 

It turns out that most oxidation-reduction reactions occur in solutions that are distinctly basic or distinctly acidic. We will cover only the acidic case in this text, because it is the most common. The detailed procedure for balancing the equations for oxidation-reduction reactions that occur in acidic solution is given below, and Example 18.5 illustrates the use of these steps. 

In using the half-reaction method, we usually begin with a skeleton ionic equation showing only the substances undergoing oxidation and reduction. In such cases, we usually do not need to assign oxidation numbers unless we are unsure whether the reaction involves oxidation-reduction. We will find that H (for acidic solutions), OH (for basic solutions), and H2O are often involved as reaaants or products in redox reactions. Unless, ... 

Complete and balance the following equations for oxidation-reduction reactions that occur in basic solution ... 

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