Asked by mae
The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.
Answers
Answered by
DrBob222
My calculator is broken. You calculate H^+ from pH = -log(H^+). I will call that value, whatever it is, x
.....................HA ==> H^+ + A^-
Initial..........0.06..........0........0
change..........-x............x..........x
equilibriium..0.06-x.......x..........x
Ka = (H^+)(A^-)/(HA)
Substitute the E line into Ka expression and solve for Ka.
Post your work if you get stuck.
.....................HA ==> H^+ + A^-
Initial..........0.06..........0........0
change..........-x............x..........x
equilibriium..0.06-x.......x..........x
Ka = (H^+)(A^-)/(HA)
Substitute the E line into Ka expression and solve for Ka.
Post your work if you get stuck.
Answered by
Yakubu Abdul-Basit
Get stuck
There are no AI answers yet. The ability to request AI answers is coming soon!