4.84
A solution with H+ = 1.2 x 10-4 a solution with OH- = 2.5 x 10 -9 A solution with pH = 4.5
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
12.85
Use this (at 25oC) : [OH-] = 10-(14-pH) ,so:[OH-] = 10-(14-10.20) = [OH-] = 10-3.80 = invlog(-3.80) = 1.6*10-4 mol/L
pH=10, so pOH=14-10=4 [OH]=10^-pOH [OH]=10^-4 [OH]=0.0001
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
A solution with H+ = 1.2 x 10-4 a solution with OH- = 2.5 x 10 -9 A solution with pH = 4.5
[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
-log[1 X 10^-4 M OH(-)] = 4 14 - 4 = 10 pH ----------------
Base. -log(3.0 X 10^-10) = pH of 9.5
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
1.70
It is a basic solution.
5.7
Use this (at 25oC) : [OH-] = 10-(14-pH) ,so:[OH-] = 10-(14-5.75) = [OH-] = 10-8.25 = invlog(-8.25) = 5.6*10-9 mol/L
12.85
12.85