The nonahydrate and other hydrated aluminium nitrates have many applications.

Aluminium nitrate is a strong oxidizing agent.

When nitronium tetranitratoaluminate is sublimed it can form anhydrous aluminium nitrate.

Aluminium nitrate can be heated at 125 C with nitrosonium or nitronium perchlorate to yield hexaperchloratoaluminates.

When aluminium ion (say as aluminium nitrate) is employed as the titrant, fluoride can be determined using the same chemistry.

Aluminium nitrate may instead be prepared by the reaction of nitric acid with aluminium(III) chloride.

Aluminium nitrate cannot be synthesized by the reaction of aluminium with concentrated nitric acid, as the aluminium forms a passivation layer.

This detection limit was determined from analysis of aluminium standards made from solutions of aluminium nitrate in poly (ethyl methacrylate) resin.

Aluminium nitrate may also be prepared a metathesis reaction between aluminium sulfate and a nitrate salt with a suitable cation such as barium, strontium, calcium, silver, or lead.

This process has the disadvantage of requiring the use of a salting-out reagent (aluminium nitrate) to increase the nitrate concentration in the aqueous phase to obtain a reasonable distribution ratio.

Aluminium nitrate is a salt of aluminium and nitric acid, most commonly existing as the crystalline hydrate, aluminium nitrate nonahydrate, Al(NO) 9HO.

The major other uses of aluminium hydroxide is as a feedstock for the manufacture of other aluminium compounds: specialty calcined aluminas, aluminium sulfate, polyaluminium chloride, aluminium chloride, zeolites, sodium aluminate, activated alumina, aluminium nitrate.