is aluminum hydroxide a solid liquid or gas
solid
title: Lye text: reacts with lyes to produce hydrogen gas. Since hydrogen is flammable, mixing a large quantity of a lye such as sodium hydroxide with aluminum in a closed container is dangerous—especially when the system is at a high temperature, which speeds up the reaction. In addition to aluminum, lyes may also react with magnesium, zinc, tin, chromium, brass or bronze—producing hydrogen gas. Lye A lye is a metal hydroxide traditionally obtained by leaching ashes (containing largely potassium carbonate or "potash"), or a strong alkali which is highly soluble in water producing caustic basic solutions. "Lye" is commonly an alternative name of title: Sodium hydroxide text: the resulting heat may cause heat burns or ignite flammables. It also produces heat when reacted with acids. Sodium hydroxide is also mildly corrosive to glass, which can cause damage to glazing or cause ground glass joints to bind. Sodium hydroxide is corrosive to several metals, like aluminium which reacts with the alkali to produce flammable hydrogen gas on contact: Careful storage is needed when handling sodium hydroxide for use, especially bulk volumes. Following proper NaOH storage guidelines and maintaining worker/environment safety is always recommended given the chemical's burn hazard. Sodium hydroxide is often stored in bottles--as in laboratories, small-scale title: Sodium hydroxide text: Sodium hydroxide Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations and hydroxide anions . Sodium hydroxide is a highly caustic base and alkali that decomposes proteins at ordinary ambient temperatures and may cause severe chemical burns. It is highly soluble in water, and readily absorbs moisture and carbon dioxide from the air. It forms a series of hydrates NaOH·"n". The monohydrate NaOH· crystallizes from water solutions between 12.3 and 61.8 °C. The commercially available "sodium hydroxide" is often this monohydrate, title: Aluminium(I) oxide text: Aluminium(I) oxide Aluminium(I) oxide is a compound of aluminium and oxygen with the chemical formula AlO. It can be prepared by heating the stable oxide AlO with elemental silicon at 1800 °C under vacuum. AlO commonly exists as a gas, since the solid state is not stable at room temperature and is only stable between 1050 and 1600 °C. Aluminium(I) oxide is formed by heating Al and AlO in a vacuum while in the presence of SiO and C, and only by condensing the products. Information is not commonly available on this compound; it is unstable, has complex high-temperature spectra, title: Aluminium chloride text: in 1993, approximately 21,000 tons were produced, not counting the amounts consumed in the production of aluminium. Hydrated aluminium trichloride is prepared by dissolving aluminium oxides in hydrochloric acid. Metallic aluminum also readily dissolves in hydrochloric acid ─ releasing hydrogen gas and generating considerable heat. Heating this solid does not produce anhydrous aluminium trichloride, the hexahydrate decomposes to aluminium hydroxide when heated: Aluminium also forms a lower chloride, aluminium(I) chloride (AlCl), but this is very unstable and only known in the vapour phase. AlCl is probably the most commonly used Lewis acid and also one of the most powerful. It