Buffer Problem, Strong acid and Strong base?

Calculate the pH of the solution resulting from the addition of 30.0 mL of .200 M HClo4 to 60.0 mL of .150M NaoH.

Answer is 12.52, just dont know how to get there

Answer:
in any acid base problem start by writing a reaction:

the net ionic equation of a strong acid with a strong base is always:

H+ + OH- --> H2O

now we have to find how many moles there are of each substance (M x L)

we have 0.030L x 0.2 M = 0.006 moles acid

we also have 0.060L x 0.150M = 0.009 moles base.

H+...+OH- --> H2O

.006...0.009

-.006.-.006

0..0.003

notice: i subtracted by the limiting factor. also notice that the water is irrelevant.

now we have 0.003 moles of base. to find pH, we need to find the Molarity. to find M, we must divide by the TOTAL volume which is 0.06+0.03 = 0.09L.

0.003 / 0.09 = 0.033 M.

now take the log of that and add 14

log (0.033) +14 = 12.52

please contact me if u need further help.

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