Which of the following statements about the pH of 0.010 M HClO4 is correct? pH=2.00, because [H+]=1.0×10−2M.

A: p H equals 2.00 , because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar .

pH=2.00, because [H+]=2.0×10−2M.

B: p H equals 2.00 , because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar .

pH>2.00, because HClO4 is a strong acid.

C: p H is greater than 2.00 , because H C l O 4 is a strong acid.

pH<2.00, because HClO4 is a weak acid.

Option B: p H equals 2.00 , because the molar concentration of H with a positive 1 charge equals 1.0 times 10 to the negative 2 power molar .

pH = 2 because [H⁺] = 1×10¯² M

Explanation:

To know which option is correct, we shall determine the pH of the 0.010 M HClO₄ solution. This can be obtained as follow:

We'll begin by calculating the concentration of the hydrogen ion [H⁺] in the solution. This is illustrated below:

HClO₄ is a strong acid and will dessociates as follow:

HClO₄ (aq) —> H⁺ (aq) + ClO₄¯ (aq)

From the balanced equation above,

1 mole of HClO₄ produced 1 mole H⁺.

Therefore, 0.010 M HClO₄ will also produce 0.010 M H⁺.

Finally we shall determine the pH of the solution. This can be obtained as follow:

Concentration of the hydrogen ion [H⁺] = 0.010 = 1×10¯² M

pH =?

pH = –Log [H⁺]

pH = –Log 1×10¯²

pH = 2

Thus,

The pH = 2

because,

[H⁺] = 1×10¯² M

Thus, option B gives the correct answer to the question.

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