Part A What is the H+ concentration for an aqueous solution with pOH = 3.26 at 2
ID: 495781 • Letter: P
Question
Part A
What is the H+ concentration for an aqueous solution with pOH = 3.26 at 25 C?
Express your answer to two significant figures and include the appropriate units.
Arrange the following aqueous solutions, all at 25 C, in order of decreasing acidity.
Rank from most acidic to most basic. To rank items as equivalent, overlap them.
pOH = 8.55
pH = 5.45
0.0023 M HCl
0.0018 M KOH
Part C
At a certain temperature, the pH of a neutral solution is 7.28. What is the value of Kw at that temperature?
Express your answer numerically using two significant figures.
Explanation / Answer
PART(A)
We know that,
pH + pOH = 14
pH = 14 - 3.26
pH = 10.74
- Log[H+] = 10.74
[H+] = 1.8 * 10-11 M
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(i) pH = 14 - pOH = 14 - 8.55 = 5.45
pH = 5.45
pH = - log[H+] = - Log(0.0023) = 2.64
pH = 14 - pOH = 14 + Log[OH] = 14 + Log(0.0018) = 11.26
Hiher the pH value smaller the acidic nature.
0.0023M HCl (1) > pOH =8.55(2) = pH = 5.45 (2) > 0.0018 M KOH (3)
PART (C)
pH = 7.28
- Log[H+] = 7.28
[H+] = 5.25 * 10-8 M
Since the solution is noted as neutral solution, [OH-] = [H+] = 5.25 * 10-8 M
Then, Kw = [H+][OH-]
Kw = 5.25 * 10-8 * 5.25 * 10-8
Kw = 2.8 * 10-15