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Chapter 14: Problem 53

What are the major species present in \(0.250 M\) solutions of each of the following acids? Calculate the \(\mathrm{pH}\) of each of these solutions. a. \(\mathrm{HClO}_{4}\) b. \(\mathrm{HNO}_{3}\)

Short Answer

Expert verified
The major species in the 0.250 M HClO₄ solution are H⁺ and ClO₄⁻ ions, with a pH of approximately 0.60. The major species in the 0.250 M HNO₃ solution are H⁺ and NO₃⁻ ions, with a pH of approximately 0.60.

Step by step solution

01

(Dissociation of HClO₄)

HClO₄ will dissociate completely in water as follows: \(HClO_{4} (aq) -> H^{+} (aq) + ClO_{4}^{-} (aq)\)
02

(Dissociation of HNO₃)

HNO₃ will dissociate completely in water as follows: \(HNO_{3} (aq) -> H^{+} (aq) + NO_{3}^{-} (aq)\) ### Step 2: Calculate the concentration of H⁺ ions ###
03

(Concentration of H⁺ ions in HClO₄ solution)

Since HClO₄ is a strong acid that dissociates completely, the concentration of H⁺ ions in the 0.250 M HClO₄ solution will be equal to the initial acid concentration: [H⁺] = 0.250 M
04

(Concentration of H⁺ ions in HNO₃ solution)

Similarly, for HNO₃, the concentration of H⁺ ions will be equal to the initial acid concentration: [H⁺] = 0.250 M ### Step 3: Calculate the pH of each solution ###
05

(pH of HClO₄ solution)

Using the pH formula, we have: pH = -log([H⁺]) = -log(0.250) ≈ 0.60
06

(pH of HNO₃ solution)

Since the concentration of H⁺ ions is the same as that in HClO₄ solution, the pH is also the same: pH = -log([H⁺]) = -log(0.250) ≈ 0.60 So, the major species present in the 0.250 M HClO₄ solution are H⁺ and ClO₄⁻ ions, with a pH of approximately 0.60. The major species present in the 0.250 M HNO₃ solution are H⁺ and NO₃⁻ ions, with a pH of approximately 0.60.

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