Asked by L.Bianchessi
A 0.035 M solution of a weak base has a pH of 10.88. What is the Kb for the acid?
Where Di I even begun**???
Where Di I even begun**???
Answers
Answered by
DrBob222
You ALWAYS start with one or all of the following:
1. balanced equation
2. ICE chart
3. think in terms of mols.
pH = 10.88 so pOH = 3.12 and OH^- = 7.58E-4
M..........BOH ==> B^+ + OH^-
initial.0.035M.....0......0
change..7.58E-4..7.58E-4..7.58E-4
equil..0.035-7.58E-4....etc
Kb = (B^+)(OH^-)/(BOH)
Substitute from the ICE chart and solve for Kb. Note that 0.035-7.58E-4 is not = 0.035
1. balanced equation
2. ICE chart
3. think in terms of mols.
pH = 10.88 so pOH = 3.12 and OH^- = 7.58E-4
M..........BOH ==> B^+ + OH^-
initial.0.035M.....0......0
change..7.58E-4..7.58E-4..7.58E-4
equil..0.035-7.58E-4....etc
Kb = (B^+)(OH^-)/(BOH)
Substitute from the ICE chart and solve for Kb. Note that 0.035-7.58E-4 is not = 0.035
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.