A certain monoprotic weak acid with Ka = 6.7 × 10-8 can be used in various industrial processes, but is no longer used in chemistry teaching labs because it tends to explode when it gets old. (a) What is the [H+] for a 0.558 M aqueous solution of this acid and (b) what is its pH?

Question

PLEASE HELP!!

DrBob222 · Answer

...........HA ==> H^+ + A^-
begin....0.558M...0.....0
change.....-x......x.....x
final...0.558-x....x.....x

Ka = (H^+))A^-)/(HA)
Substitute the ICE chart values I made into the Ka expession and solve for H^+.
b) pH = -log(H^+)

Adrianna · Answer

Thank you so much!!

Anonymous · Answer

I HAVE NO F$#@ING IDEA!!!!!!!!!!!!!

merhawit · Answer

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