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Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
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Calculate the pH of each of the following strong acid

Chapter , Problem 16.43

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QUESTION:

Calculate the pH of each of the following strong acid solutions: (a) 8.5 * 10-3 M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of 0.250 M HClO4 diluted to 50.0 mL, (d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCl.

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QUESTION:

Calculate the pH of each of the following strong acid solutions: (a) 8.5 * 10-3 M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of 0.250 M HClO4 diluted to 50.0 mL, (d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCl.

ANSWER:

Problem 16.43Calculate the pH of each of the following strong acid solutions: (a) 8.5 x 10 M HBr, (b) 1.52 g of -3HNO in 575 mL of solution, (c) 5.00 mL of 0.250 M HClO diluted to 50.0 mL, (d) a solution 3 4formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCl. Step-by-step solution Step 1 of 4 (a)Strong acids ionize completely in water, so HBr ionizes completely in water. So, the ionization of -38.5 x 10 M hydrobromic acid is given by the equation: HBr(aq) + H O(2) H O (a3 + + Br (aq) -3 -3 -3 8.5 x 10 M 8.5 x 10 M 8.5 x 10 M + - -3That it produces H O , Br3ions each with a concentration of 8.5 x 10 M [H O ] = [Br ] - 3 -3 = 8.5 x 10 MThus, the concentration of will be H O 8.5 x 10 M. + -3 3pH of the solution is defined as the negative base-10 logarithm of the hydrogen ionconcentration (mol/L). pH = - log [H O ] + 3 -3 = - log ( 8.5 x 10 ) = 2.07 -3Thus, pH of the 8.5 x 10 M HBr solution is .

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