A buffer solution with a volume of 0.0250 L consists of 0.61 M iodous acid (HIO2),...
A buffer solution with a volume of 0.0250 L consists of 0.61 M iodous acid (HIO2), a weak acid, plus 0.61 M lithium iodite (LiIO2). The acid dissociation constant of iodous acid, Ka, is 3.2 ✕ 10−5. Determine the pH of the buffer solution after the addition of 0.0034 mol sodium hydroxide (NaOH), a strong base. (Assume no change in solution volume.)
can u solve with an ice table? thank you.
Homework Answers
Answer:
To determine pH
Consider,
Moles of HIO2 = 0.61*0.0250
= 0.01525
HIO2 left after adding KOH = 0.01525 - 0.0034
= 0.01185 mol
IO2- = 0.01525 + 0.0034
= 0.01865
Now consider,
3.2*10^-5 = 0.01525*[H3O+] / 0.01185
[H3O+] = 3.9*10^-5
pH = -log(3.9*10^-5)
pH = 4.41
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