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Section 3: What is pH?

What is pH?

1.

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Why is it possible to derive the ion product constant for water, but not for aqueous acids?
A)At a given temperature, aqueous acids have constant concentrations.
B)Aqueous acids never reach equilibrium.
C)The concentration of pure water is constant.
D)Water does not ionize completely.
2.
pH is defined as __________.
A)log [H+]
B)-log [H+]
C)log [OH-]
D)-log [OH-]
3.
A solution of pH = 2.1 would be described as __________.
A)distinctly basic
B)slightly basic
C)slightly acidic
D)distinctly acidic
4.
When a solution has a pH of 4, what is the pOH of that solution?
A)10
B)4
C)18
D)7
5.
At 298 K, pure water has a pH of __________.
A)0
B)14
C)-14
D)7
6.
What is the concentration of hydrogen ions in a solution that has a pH of 4.32?
A)4.8 x 10-5M
B)6.2 x 10-4M
C)5.1 x 10-4M
D)8.6 x 10-5M
7.
Calculate the pH of 0.075M KOH.
A)10.4
B)11.12
C)11.46
D)12.88
8.
Calculate the pH of a solution that has a [OH-] = 2.50 x 10-4M.
A)0.4
B)3.6
C)-3.6
D)10.4
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