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Oxidizing Reducing Calculator
A substance that removes electrons from another reactant in a redoxchemical reaction
Defination / Uses
In a redoxchemical reaction, an oxidation state (also known as an oxidant, oxidizer, or oxidiser) is a substance that removes electrons from another reactant. The oxidant is "reduced" by receiving electrons from the reactant, while the reactant is "oxidised" by losing electrons. Although oxygen is the most well-known oxidant, it is only one of many.
Our Oxidizing - Reducing Calculator help to calculate the equivalent weight of oxidising / reducing agents.
In a chemical process, an oxidising agent, also known as an oxidant, obtains electrons and is reduced. The oxidising agent, also known as the electron acceptor, is generally in one of its higher oxidation states since it will receive electrons and be reduced. Halogens, potassium nitrate, and nitric acid are examples of oxidising agents.
In a chemical process, a reducing agent, also known as a reductant, loses electrons and is oxidised. When a reducing substance is in one of its lower oxidation states, it is referred to as an electron donor. Because it loses electrons in the redox reaction, a reducing agent becomes oxidised. Earth metals and formic acid are examples of reducing agents. Use the upper given formula for manual calculations. No sign-up, registration OR captcha is required to use this tool.