Homework Answers
All are strong acids dissociates completely into ions . As all are monoprotic acids, the concentration of hydronium ion formed on dissociation is equal to concentration of acid. That is
[H3O+] = [acid]
pH is given as
pH = -log [H3O+]
At 25oC [H3O+] [OH-] = 10-14
[OH-] = 10-14/[H3O+]
On the basis of above formula let us do calculation for each part
a) [H3O+] = 0.0150 M
pH = -log (0.0150) = 1.82
[OH-] = 10-14/0.0150 = 6.6 x 10-13 M
b ) Here the concentration of [H3O+] from acid is very less than the hydronium ions from water so the concentration of hydronium ion is given as [H3O+] ~ 10-6.99 M
pH = -log (10-6.99) = 6.99
[OH-] = 10-14/10-6.99= 9.78 M
c) [H3O+] = 0.0226 M
pH = -log (0.0226) = 1.64
[OH-] = 10-14/0.0226 = 4.4 x 10-13 M
a) [H3O+] = 0.0017 M
pH = -log (0.0017) = 2.77
[OH-] = 10-14/0.0017 = 5.8 x 10-12 M
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