A report on Corrosive substance, Nitric acid and Ammonia

The international pictogram for corrosive chemicals.

Fuming nitric acid contaminated with yellow nitrogen dioxide

Ball-and-stick model of the diamminesilver(I) cation, [Ag(NH3)2]+

The international transport pictogram for corrosives.

Two major resonance representations of HNO3

Ball-and-stick model of the tetraamminediaquacopper(II) cation, [Cu(NH3)4(H2O)2](2+)

This high-pressure reactor was built in 1921 by BASF in Ludwigshafen and was re-erected on the premises of the University of Karlsruhe in Germany.

Ammoniacal Gas Engine Streetcar in New Orleans drawn by Alfred Waud in 1871.

The X-15 aircraft used ammonia as one component fuel of its rocket engine

Anti-meth sign on tank of anhydrous ammonia, Otley, Iowa. Anhydrous ammonia is a common farm fertilizer that is also a critical ingredient in making methamphetamine. In 2005, Iowa used grant money to give out thousands of locks to prevent criminals from getting into the tanks.

The world's longest ammonia pipeline (roughly 2400 km long), running from the TogliattiAzot plant in Russia to Odessa in Ukraine

Hydrochloric acid sample releasing HCl fumes, which are reacting with ammonia fumes to produce a white smoke of ammonium chloride.

Production trend of ammonia between 1947 and 2007

Main symptoms of hyperammonemia (ammonia reaching toxic concentrations).

Ammonia occurs in the atmospheres of the outer giant planets such as Jupiter (0.026% ammonia), Saturn (0.012% ammonia), and in the atmospheres and ices of Uranus and Neptune.

It is a highly corrosive mineral acid.

- Nitric acid

Although common in nature—both terrestrially and in the outer planets of the Solar System—and in wide use, ammonia is both caustic and hazardous in its concentrated form.

- Ammonia

Some corrosives, such as nitric acid and concentrated sulfuric acid, are strong oxidizing agents as well, which significantly contributes to the extra damage caused.

- Corrosive substance

Some concentrated weak bases, such as ammonia when anhydrous or in a concentrated solution

- Corrosive substance

It combines with acids to form salts; thus with hydrochloric acid it forms ammonium chloride (sal ammoniac); with nitric acid, ammonium nitrate, etc. Perfectly dry ammonia gas will not combine with perfectly dry hydrogen chloride gas; moisture is necessary to bring about the reaction.

- Ammonia

Upon adding a base such as ammonia, the color turns orange.

- Nitric acid

2 related topics with Alpha

Acid

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Molecule or ion capable of either donating a proton , known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid.

Acetic acid, a weak acid, donates a proton (hydrogen ion, highlighted in green) to water in an equilibrium reaction to give the acetate ion and the hydronium ion. Red: oxygen, black: carbon, white: hydrogen.

Hydrochloric acid (in beaker) reacting with ammonia fumes to produce ammonium chloride (white smoke).

This is an ideal titration curve for alanine, a diprotic amino acid. Point 2 is the first equivalent point where the amount of NaOH added equals the amount of alanine in the original solution.

Carbonated water (H2CO3 aqueous solution) is commonly added to soft drinks to make them effervesce.

Aspirin (acetylsalicylic acid) is a carboxylic acid

Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.

An example is boron trifluoride (BF3), whose boron atom has a vacant orbital that can form a covalent bond by sharing a lone pair of electrons on an atom in a base, for example the nitrogen atom in ammonia (NH3).

Examples of strong acids are hydrochloric acid (HCl), hydroiodic acid (HI), hydrobromic acid (HBr), perchloric acid (HClO4), nitric acid (HNO3) and sulfuric acid (H2SO4).

Sulfuric acid

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Mineral acid composed of the elements sulfur, oxygen and hydrogen, with the molecular formula H2SO4.

Solid state structure of the [D3SO4]+ ion present in [D3SO4]+[SbF6]−, synthesized by using DF in place of HF. (see text)

Acidic drain cleaners usually contain sulfuric acid at a high concentration which turns a piece of pH paper red and chars it instantly, demonstrating both the strong acidic nature and dehydrating property.

An acidic drain cleaner can be used to dissolve grease, hair and even tissue paper inside water pipes.

John Dalton's 1808 sulfuric acid molecule shows a central sulfur atom bonded to three oxygen atoms, or sulfur trioxide, the anhydride of sulfuric acid.

Drops of 98% sulfuric acid char a piece of tissue paper instantly. Carbon is left after the dehydration reaction staining the paper black.

Superficial chemical burn caused by two 98% sulfuric acid splashes (forearm skin)

Similarly, reacting sulfuric acid with potassium nitrate can be used to produce nitric acid and a precipitate of potassium bisulfate.

Reacting the ammonia produced in the thermal decomposition of coal with waste sulfuric acid allows the ammonia to be crystallized out as a salt (often brown because of iron contamination) and sold into the agro-chemicals industry.

The standard first aid treatment for acid spills on the skin is, as for other corrosive agents, irrigation with large quantities of water.