Al(OH)3 (s) + OH- (aq) -------> [Al(OH)4]- (aq)
Aluminium hydroxide undergoes further reaction with hydroxide ion to from a complex ion, which is of course, soluble in water.
Some other metal hydroxides also have similar reaction, like zinc hydroxide, and lead (II) hydroxide.
2 Al + 6 H2O > 2 Al(OH)3 + 3 H2 Al(OH)3 + NaOH > Na+ + [Al(OH)4]- __________________________________________________________________ 6H2O(l)+2Al(s)+2NaOH(aq)--------------- 2NaAl(OH)4(aq)+3H2(g)
Sodium hydroxide reacts with aluminum, corroding the metal and producing hihgly flammable hydrogen gas.
Since aluminium oxide is an amphoteric oxide, it does react with the alkali sodium hydroxide in an aqueous medium. It is an acid base reaction.
Sodium Hydroxide in contact with some metals ( Aluminium , Magnesium , Zinc ) reacts to produce flammable and potentially explosive Hydrgen Gas. Aluminium is actually a very reactive metal that is unusual as it has layer of oxide ( Al2O3 ) on the surface. This oxide is soluble in base forming an aluminate exposing the Aluminium surface which reacts.
Negative. Aluminium will react with sodium hydroxide or hydrochloric acid. Trying to make a works bomb?
No, adding solid sodium hydroxide to neutralize hydrochloric acid (HCl) would not cause sodium chloride to redissolve. The reaction between sodium hydroxide and hydrochloric acid forms water and sodium chloride, which remains in its dissolved form. The addition of solid sodium hydroxide would simply further neutralize the acid and increase the concentration of the resulting sodium chloride solution.
Aluminium doesn't react with sodium bicarbonate.Aluminium react with sodium hydroxide.
2 Al + 6 H2O > 2 Al(OH)3 + 3 H2 Al(OH)3 + NaOH > Na+ + [Al(OH)4]- __________________________________________________________________ 6H2O(l)+2Al(s)+2NaOH(aq)--------------- 2NaAl(OH)4(aq)+3H2(g)
Sodium hydroxide must be dissociated in water.
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Aluminium hydroxide = Al(OH)3 , and Zinc hydroxide = Zn(OH)2 , is redissolved in excess Sodium hydroxide = NaOH (in water solution) : Al(OH)3 + NaOH + H2O ----> NaAl(OH)4 Zn(OH)2 + NaOH + H2O ----> Na2Zn(OH)4
The reaction of zinc nitrate and excess sodium hydroxide begins with precipitation of zinc hydroxide ( Zn(OH)2 ), followed by dissolvement after adding excess sodium hydroxide ( 2 OH- ) to formation of zinc aat-ions ( [Zn(OH)4]2- )
Ammonia
There is no reaction , because of the Common Ion Effect. The Common Ion is the Hydroxide.
Aluminium foil, sodium hydroxide
Sodium hydroxide reacts with aluminum, corroding the metal and producing hihgly flammable hydrogen gas.
Test: Add aqueus sodium carbonate solution, then warm it. Observation: Formation of white precipitate. Deduction: The presence of aluminum ions, Al3+ Or Test: Observation: Add aqueous sodium hydroxide White precipitate occur Add aqueous sodium hydroxide (excess) & warm White precipitate solute Test with red litmus paper Changes red - blue Deduction: The presence of aluminum ions, Al3+