strength of acids and bases (1 Viewer)

[CM_Tutor]

Originally posted by t-i-m-m-y
CM-tutor: oops i didn't see the "teacher" status but i see it now.hehehe

Yeah, Lazarus 'promoted' me about a month ago

 

[xiao1985]

Originally posted by CM_Tutor
No. Arrhenius definition is still based on the formation of new ions from a net uncharged, covalently bonded molecule, so it's still an ionisation - in fact, the first example I wrote of ionisation uses the Arrhenius definition.

Oh well, alchemists will certain hold more BBQs - they just won't de free to first years!

ohhh.... and because NaOH is ionically bonded instead of covalently bonded, therefore, there are already charges on individual ions before they dissolve in water, right?? that's y they are called dissociation ^^

mg, visitin bos frequently does help, aprt from i had to stare at screen at fisher for 5 hrs straight =( pffttt

*whines

my eyes r sore ='(

 

[BlackJack]

Well, it is helpful to think of acids as creating new ions of H₃O⁺ when you dissoolve them. H⁺ do not exist by themselves and must bind to water. Hence ionisation.
In bases like NaOH, there is no new ion created when you dissolve it. You only break the ionic attraction. Hence dissociation.

Turn down brightness and contrast. Mine are very sensitive so I usually turn them right down.

 

[xiao1985]

Originally posted by BlackJack

Turn down brightness and contrast. Mine are very sensitive so I usually turn them right down.

lolz, reminds of a jk on my usyd diary:

y ain't there a knob on tv which controls intellegience?? there's one called brightness, but it doens't work... =p