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ritwik06
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Why does oxidizing nature of nitric acid gets reduced on dilution?
ritwik06 said:Why does oxidizing nature of nitric acid gets reduced on dilution?
chemisttree said:What do you mean by 'oxidizing nature'? Rate of oxidation?
Stevedye56 said:Do you mean why is a subastance being oxidized the reducing agent?
ritwik06 said:I am sorry! I got it. Thanks a lot to all of you!
chemisttree said:What is the oxidation # for nitrogen in the nitrate ion? Is it unusual?
no, H+ itself gets reduced while the other substance loses e- and gets oxidizedritwik06 said:H+ ions are responsible for reducing nature, so why oxidizing nature decreases?
chemisttree said:Oxygen usually has an oxidation number (I'll call it a 'charge') of -2. There are three of them (oxygens in nitrate) and there is one negative charge left over. What is the charge on nitrogen required to balance all but one of these negative charges?
Nitrogen usually has an oxidation number of -3...
chemisttree said:The oxidative property of nitric acid comes from the nitrate ion. The proton doesn't counteract this at all. I don't know of any reactions where H+ is a reducing agent or where it could lead to reduction.
ritwik06 said:...But sir, please do tell me that when nitrogen in nitrate has oxidation # +5, then how does it effect the oxidizing nature?
Nitric acid (HNO3) is a strong mineral acid commonly used in the field of chemistry. It is a colorless liquid with a pungent odor and is highly corrosive. Nitric acid is commonly used in the production of fertilizers, explosives, and dyes. It is also used in various laboratory experiments and industrial processes.
Nitric acid is a strong acid with a pH level of less than 2. It is highly corrosive and can cause severe burns on contact with the skin. It is also a strong oxidizing agent, meaning it can easily react with other substances and release oxygen. Nitric acid is soluble in water and forms a clear, colorless solution. It has a boiling point of 83°C and a density of 1.5 g/mL.
Nitric acid is typically produced through the oxidation of ammonia. In this process, ammonia gas is mixed with air and passed through a catalyst at high temperatures. This results in the formation of nitrogen dioxide, which is then dissolved in water to produce nitric acid. The production of nitric acid can also be achieved through the reaction of sulfuric acid with sodium nitrate.
Due to its corrosive nature, nitric acid can cause severe burns on contact with the skin and eyes. It can also irritate the respiratory system if inhaled. In addition, nitric acid is a strong oxidizing agent and can react violently with other substances, potentially causing explosions. Proper safety precautions, such as wearing protective gear and working in a well-ventilated area, should always be taken when handling nitric acid.
In laboratory experiments, nitric acid is often used as a strong acid to neutralize basic solutions and as an oxidizing agent to break down organic compounds. It is also used in titration experiments to determine the concentration of a substance. Additionally, nitric acid is commonly used to etch metals and as a reagent in the synthesis of various compounds.