Calculate the pH of the solution of 0.112M CsBrO. I know Cs+ and Br- are spectator ions but I can't figure out how to solve this.
No volume was given nor is it necessary to solve a weak acid/base problem when it is not a mixture. The final pH is 10.82 I just need the steps to solve it.
HBrO , Ka = 2.8 x 10^-9
Kb = Kw / Ka
Kb = 1.0 x 10^-14 / 2.8 x 10^-9
Kb = 3.57 x 10^-6
CsBrO -----------------> Cs+ + BrO-
Cs+ is the only spectator ion . BrO - ion will particiapte in hydrolysis because it came from weak acid
BrO- + H2O ------------------> HBrO + OH-
0.112 0 0 -------------> initial
-x + x + x ------------> change
0.112-x x x ------------------> equilibrium
Kb = [HBrO][OH-]/[BrO-]
3.57 x 10^-6 = x^2 / 0.112-x
x^2 + 3.57 x 10^-6 x - 4.0 x 10^-7 = 0
by solving this
x = 6.32x 10^-4
x = [OH-] = 6.32 x 10^-4 M
pOH = -log [OH-]
pOH = -log (6.32 x 10^-4)
pOH = 3.20
pH + pOH = 14
pH + 3.20 = 14
pH = 10.8 --------------------------> answer
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