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1) What is the pH of the solution with a hydronium concentration [H3O+]
1.47 x 10-4?
What is the pOH of this solution?
pH = -log (1.47 x 10-4)
= 3.83
pOH = 14 - pH = 14 -
3.83 = 10.17
2) What is the pOH of the solution with a hydroxyl concentration [OH-] 2.98 x
10-2?
What is the hydronium concentration [H3O+]
of this solution?
pOH = -log (2.98 x 10-2)
= 1.53
hydronium concentration [H3O+]
= 1 x 10-14
= 3.37 x 10-13
2.98 x 10-2
OR
pH = 14- pOH = 14 - 1.53 = 12.47
hydronium concentration [H3O+]
= antilog -12.47 = 3.38 x 10-13
3) What is the hydronium concentration [H3O+] of a
solution with a pH of 7.84?
What is the hydroxyl concentration [OH-] of this
solution?
hydronium concentration [H3O+]
= antilog -7.84 = 1.45 x 10-8
hydroxyl concentration [OH-]
= 1 x 10-14 = 6.90
x 10-7
1.45 x 10-8
OR pOH = 14-pH = 14 - 7.84 =
6.16
hydroxyl concentration
[OH-] = antilog -6.16 = 6.9 x 10-7
4) What is the hydroxyl concentration [OH-] of a solution with a pH of 3.76?
pOH = 14 - pH = 14 - 3.76 =
10.24
hydroxyl concentration [OH-] =
antilog -10.24 = 5.75 x 10-11
5) What is the hydronium concentration [H3O+] of a
solution with a pOH of 2.47?
pH = 14 - pOH = 14 - 2.47 =
11.53
hydronium concentration [H3O+]
= antilog -11.53 = 2.95 x 10-12
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