I saw a formula

 

sodium hydroxide(aq) + aluminium(s) + water (l)

to form something.

Actually, it is to damage something.

But for acid

hydrogen chloride(aq)+Al(s)

to damage something.

Why does sodium hydroxide need to get some water but hydrochloric acid doesn't need to? Doesn't the sodium hydroxide is already in aqueous form and is in water?

maybe because the sodium hydroxide is a limiting reagent. just a guess

well, one can say that acid anhydrides aren't all that corrosive but they will hit water on contact with the body forming incredibly conc acids.

I still don't know,sorry. Would you please explain it further more?

By the way, the book said hydrofluoric acid is less acidic than hydrochloric acid since it has a too strong electronegetivity energy, so it's ionization energy is less. Is that rue? It said HF has a fewer number of F- ions compare to the same mole of HCl solution.

the trend with halide acids is that the higher the halogen the less ionization occurs. if you take any given volume of all halogen acids at a certain molarity, you will find that the acidity of HI>HBr>HCl>HF

HI is the strongest acid in halogens but not powerful than HF when reacting with compound?

HI-large amount but all are weak. HF-small amount but all are strongest.

Am I right?

But why do alkaline need additional water as reactant react with?

water`s needed as the ion carrier in these instances.

I think it's just a mistake, if you have an aqueous solution, then water is in excess anyway.

HI is the strongest acid in halogens but not powerful than HF when reacting with compound?

it depends on what you're attacking.

dont all acids and alkalines contain water, or wouldnt they just be salt crystals?

 

js

"acid" and "alkaline" are terms referring to aqueous solutions of compounds that (respectfully) donate and accept hydronium ions

Which is what i was meaning, lol.

 

js