Explanation Strong acids, by definition, completely ionize in solution. Because we can (in nearly all cases) ignore the contribution of the autoionization of water, the concentration of in a strong acid solution is equal to the concentration of [H 3 O + ] the strong acid. pH is defined as the negative of the log of the hydronium ion concentration: pH=-log[H 3 O + ] Given: a. pH = 2.50 b. pH = 1.50 c. pH = 0.50 Calculation a. pH = 2.50 pH=-log[H 3 O + ] [H 3 O + ]=10 −pH =10 −250 =0.0032M HClO 4 is a strong acid, hence ionizes completely. [H 3 O + ]=[HC1O 4 ]=0.0032M Thus, number of moles of HClO 4 in 0.500 L solution (n) is given by, n=0 .0032× 500 1000 =0 .0016 moles Molar mass of HClO 4 is 100.46. Hence, mass of 0.0016 moles of HClO 4 is, m=0.0016×100.46=0.16g b. pH = 1.50 pH=-log[H 3 O + ] [H 3 O + ]=10 −pH =10 −150 =0...

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ISBN: 9780321834683

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 17, Problem 62E

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To determine: Mass of HClO₄ required in 0.500 L of solution to obtain a solution with each of the given pH value.

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Chapter 17, Problem 61E

Chapter 17, Problem 63E

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Chapter 17 Solutions

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Mass of HClO 4 required in 0.500 L of solution to obtain a solution with each of the given pH value.

Solution Summary: The author calculates the mass of HClO 4 required in 0.500 L of solution to obtain a solution with each of the given pH values.

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To determine: Mass of HClO₄ required in 0.500 L of solution to obtain a solution with each of the given pH value.

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Chapter 17 Solutions

Mass of HClO 4 required in 0.500 L of solution to obtain a solution with each of the given pH value.

Solution Summary: The author calculates the mass of HClO 4 required in 0.500 L of solution to obtain a solution with each of the given pH values.

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To determine: Mass of HClO4 required in 0.500 L of solution to obtain a solution with each of the given pH value.

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Chapter 17 Solutions

To determine: Mass of HClO₄ required in 0.500 L of solution to obtain a solution with each of the given pH value.