Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction. c. Cr(OH)3(𝑠)⟶CrO42−(𝑎𝑞)

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Identify the oxidation states of chromium in Cr(OH)_3 and CrO_4^{2-}.

Determine whether the half-reaction is an oxidation or a reduction by comparing the oxidation states.

Balance the chromium atoms on both sides of the equation.

Balance the oxygen atoms by adding H_2O molecules to the appropriate side.

Balance the hydrogen atoms by adding OH^- ions to the appropriate side and ensure the charge is balanced.

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주요 개념

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Half-Reactions

Half-reactions are equations that show either the oxidation or reduction process occurring in a redox reaction. They represent the transfer of electrons, with oxidation involving the loss of electrons and reduction involving the gain of electrons. In this context, balancing half-reactions is essential to ensure that both mass and charge are conserved.

Oxidation and Reduction

Oxidation is defined as the process where a substance loses electrons, resulting in an increase in oxidation state, while reduction is the gain of electrons, leading to a decrease in oxidation state. Identifying whether a half-reaction is an oxidation or reduction is crucial for understanding the overall redox process and for balancing the reaction correctly.

Basic Solution Conditions

In basic solutions, the presence of hydroxide ions (OH⁻) influences the balancing of half-reactions. When balancing in basic conditions, it is often necessary to add OH⁻ ions to neutralize any H⁺ ions that may appear during the balancing process. This ensures that the final balanced equation accurately reflects the conditions of the reaction.