Multiple Choice
Which statement best describes the behavior of a strong acid such as in water when calculating pH?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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What is the pH of a M solution of hydrobromic acid, HBr, assuming it behaves as a strong acid and water autoionization is negligible?
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Verified step by step guidance1
Recognize that hydrobromic acid (HBr) is a strong acid, which means it completely dissociates in water. Therefore, the concentration of HBr equals the concentration of hydrogen ions, \([\mathrm{H}^+]\).
Write the dissociation equation: \(\mathrm{HBr} \rightarrow \mathrm{H}^+ + \mathrm{Br}^-\), so \([\mathrm{H}^+] = 0.000100\,M\).
Recall the formula for pH: \(\mathrm{pH} = -\log[\mathrm{H}^+]\).
Substitute the hydrogen ion concentration into the pH formula: \(\mathrm{pH} = -\log(0.000100)\).
Calculate the logarithm to find the pH value, which will give you the acidity level of the solution.
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