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high Ka doesnt mean equilibrium bc Ka isnt a measure of eq, u generally use Ka equations for weak acids because they don't completely disocciate so u cant just plug the [H+] value into -log[H+] to get the pH, if that makes sense. but u can do that with strong acids. so for weak acids = use Ka...

WHAT i think ur mixing it up with something else Ka = how readily sum disociates high Ka = disociates so readily its crazy = strong acid strong acid = HCl = dissociates completely into H+ and Cl- = therefore the high Ka is justified HCl ≠ equilibrium rxn

huh no they have like rlly rlly high Ka values

NO.

don't take my word for it i might be wrong, we weren't tested on it so i never practiced it

yep exactly right, the higher the Ka the more readily it dissociates which makes sense for strong acids compared to weak acids and fml i just realised i got a question on that wrong in my trials

yeah i think its double arrow for net ionics

high Ka = strong acid. Low pKa = strong acid. think of it like [H+] concentration vs pH, high H conc = low pKa

well yeah generally w/ ppt or dissolution equations there's a double arrow from the solid to the disassociated ions

yeah so u get the most accurate conc.

oh shit i totally misread ur post i swear I'm dyslexic

yeah u should check with ur teacher specifically tho bc some schools only got to go thru half of mod 7 before their trials but def memorise it just in case arr limitations: yeah so that ammonia ammonium rxn is bc his theory couldn't explain the amphoteric nature of substances. he also couldn't...

okay wonderful keep going I'm reading

are we in America rn

THE STUTTERING NAHH

in what world.

i thought u meant mine and i started laughing, damn he's changed a lot then

ben 10 back at it again

stfu please

ud think they woulda returned him by now