Nitric Acid Production and Safety Procedures

The temperature for preparing nitric acid should not exceed 200°C to avoid decomposition and hard crust formation.

Glass apparatus is essential for preparing nitric acid due to the corrosive nature of its vapors.

KNO3 reacts with H2SO4 to produce KHSO4 and HNO3.

Pure nitric acid is colorless; commercial samples are yellowish due to dissolved nitrogen dioxide.

Use proper safety equipment, correct reagents & quantities to avoid damage and ensure proper reaction.

A method used to manufacture nitric acid on a large scale.

Ammonia ($NH_3$) reacts with oxygen ($O_2$) in the presence of a catalyst to form nitrogen monoxide ($NO$).

Nitrogen monoxide ($NO$) is further oxidized by oxygen ($O_2$) to form nitrogen dioxide ($NO_2$).

Nitrogen dioxide ($NO_2$) reacts with water ($H_2O$) and oxygen ($O_2$) to produce nitric acid ($HNO_3$).

Heating nitric acid produces brown fumes due to its instability and decomposition.

Nitric acid reacts with carbon to produce carbon dioxide, water, and nitrogen dioxide.

Nitric acid reacts with sulfur to produce sulfuric acid, water, and nitrogen dioxide.

Most metals react with nitric acid, except for gold and platinum.

Copper reacts with nitric acid to produce copper(II) nitrate, water, and nitrogen dioxide (red-brown fumes).

Iron sulfate reacts with concentrated sulfuric acid and nitric acid. Produces iron sulfate nitrate, water, and other compounds.

Sulphuric acid is commonly referred to as the "king of chemicals" due to its extensive industrial use and importance.

Sulphuric acid was historically known as "oil of vitriol" because it was first produced by distilling green vitriol, a hydrated iron sulfate.

Sulphur dioxide (SO₂) can be produced by roasting iron pyrite (FeS₂) in the presence of oxygen. This process involves the oxidation of iron pyrite to iron oxide and the release of sulphur dioxide.

Sulphur dioxide (SO₂) can be produced by burning elemental sulphur in the presence of oxygen. This reaction involves the direct oxidation of sulphur to sulphur dioxide.

When sulphur trioxide (SO₃) reacts with water, it forms sulphuric acid (H₂SO₄).

The reaction between sulfur trioxide (SO₃) and water is highly exothermic, leading to the formation of a dense sulfuric acid mist that is difficult to condense.

Oleum is a mixture of sulfur trioxide (SO₃) dissolved in concentrated sulfuric acid (H₂SO₄). It has the chemical formula H₂S₂O₇ and is also known as pyrosulfuric acid.

Sulfur dioxide (SO₂) is absorbed in concentrated sulfuric acid to form oleum (pyrosulfuric acid) through the reaction: SO₃ + H₂SO₄ → H₂S₂O₇.

Oleum is diluted with a specific amount of water to produce sulfuric acid. The reaction is: H₂S₂O₇ + H₂O → 2H₂SO₄.

Sulfur dioxide (SO₂) is oxidized to sulfur trioxide (SO₃) in the presence of a catalyst. The reaction is: 2SO₂ + O₂ → 2SO₃. This is a key step in the production of sulfuric acid.

The chemical formula for sulfuric acid is H₂SO₄.

Sulfuric acid is a strong dibasic acid, meaning it can donate two hydrogen ions (H+) per molecule.

Sulfuric acid is non-volatile, which means it doesn't easily evaporate or vaporize.

Sulfuric acid reacts with certain metals, like copper, to produce metal sulfates, water, and sulfur dioxide gas (SO₂).

Sulfuric acid reacts with organic compounds like hydrogen sulfide (H₂S) producing sulfur, water, and sulfur dioxide gas (SO₂).

A substance that removes chemically bound water molecules from a compound, resulting in a chemical change and the formation of new products.

A substance that removes moisture from gases or compounds through physical processes without altering their chemical composition.

A drying agent removes moisture through physical processes without altering the chemical composition of the substance, while a dehydrating agent removes chemically bound water molecules from a compound, resulting in a chemical change and the formation of new products.

Sulfuric acid forms a white precipitate of barium sulfate when reacted with barium chloride solution, and it turns orange acidified potassium permanganate solution colorless when sulfur dioxide is produced.

The reaction between hydrogen sulfide (H₂S) and sulfuric acid (H₂SO₄) produces sulfur (S), water (H₂O), and sulfur dioxide (SO₂).

The reaction of potassium dichromate (K₂Cr₂O₇) with sulfur dioxide (SO₂) in the presence of sulfuric acid (H₂SO₄) results in a green solution. This reaction demonstrates SO₂'s reducing properties, as it reduces the dichromate ion (Cr₂O₇²⁻) to the chromic ion (Cr³⁺), which is green in solution.

Sulfur dioxide (SO₂) acts as a reducing agent in the reaction with potassium dichromate (K₂Cr₂O₇), reducing the orange dichromate ion (Cr₂O₇²⁻) to the green chromic ion (Cr³⁺). This indicates that SO₂ donates electrons to the dichromate ion, causing its reduction.

The reducing nature of sulfur dioxide (SO₂) allows it to dissolve certain metals, a process known as leaching. SO₂ reacts with water to form sulfurous acid, which then releases nascent hydrogen (H). This nascent hydrogen is a powerful reducing agent that can react with metals, dissolving them.

Sulfur dioxide (SO₂) is used as a bleaching agent for delicate materials, particularly flowers, because of its reducing property. It is mild enough to bleach delicate materials without damaging them.

Nascent hydrogen is a highly reactive form of atomic hydrogen produced during chemical reactions. It is not a stable species and readily participates in reduction reactions. In the context of SO₂, nascent hydrogen is formed when SO₂ reacts with water and acts as a reducing agent.