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Chapter 13: Problem 55

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. HNO_3

Short Answer

Expert verified
The major species present in the 0.250 M solutions of both perchloric acid (HClO₄) and nitric acid (HNO₃) are H⁺ and their corresponding anions, ClO₄⁻ and NO₃⁻, respectively. The pH of both solutions is approximately 0.60.

Step by step solution

01

Perchloric acid dissociates completely in water as follows: \[ \mathrm{HClO}_{4} \rightarrow \mathrm{H}^{+} + \mathrm{ClO}_{4}^{-} \] Since it is a strong acid, we assume 100% dissociation. #Step 2: Find the concentration of H₃O⁺ ions formed#

Our given initial concentration of HClO₄ is 0.250 M. Since the acid dissociates completely, the concentration of H⁺ ions formed in the solution will be equal to that of the HClO₄, which is 0.250 M. #Step 3: Calculate the pH of the solution#
02

The pH of a solution is calculated using the following formula: \[ \mathrm{pH} = -\log[\mathrm{H}^{+}] \] Where [H⁺] is the concentration of H+ ions in the solution. Now, substitute the value of [H⁺] in the formula: \[ \mathrm{pH} = -\log(0.250) \] Use a calculator to find the pH: \[ \mathrm{pH} \approx 0.60 \] b. HNO₃ #Step 1: Write the dissociation equation of HNO₃#

Similarly, nitric acid dissociates completely in water as follows: \[ \mathrm{HNO}_{3} \rightarrow \mathrm{H}^{+} + \mathrm{NO}_{3}^{-} \] Assuming 100% dissociation due to the strong nature of the acid. #Step 2: Find the concentration of H₃O⁺ ions formed#
03

Given initial concentration of HNO₃ is 0.250 M. Once again, the concentration of H⁺ ions formed in the solution is the same as that of the acid, which is 0.250 M. #Step 3: Calculate the pH of the solution#

Use the same pH formula as before: \[ \mathrm{pH} = -\log[\mathrm{H}^{+}] \] Substitute the value of [H⁺] in the formula: \[ \mathrm{pH} = -\log(0.250) \] Using a calculator, find the approximate pH: \[ \mathrm{pH} \approx 0.60 \] In conclusion, the major species present in the solutions are the corresponding ions of the acids, and the pH of both the 0.250 M HClO₄ and 0.250 M HNO₃ solutions is approximately 0.60.

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Most popular questions from this chapter

At \(25^{\circ} \mathrm{C},\) a saturated solution of benzoic acid \(\left(K_{a}=6.4 \times\right.\) \(10^{-5}\) ) has a pH of \(2.80 .\) Calculate the water solubility of benzoic acid in moles per liter.

Calculate \(\left[\mathrm{OH}^{-}\right],\left[\mathrm{H}^{+}\right],\) and the \(\mathrm{pH}\) of \(0.20 M\) solutions of each of the following amines. a. triethylamine \(\left[\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{N}, K_{\mathrm{b}}=4.0 \times 10^{-4}\right]\) b. hydroxylamine (HONH \(\left._{2}, K_{\mathrm{b}}=1.1 \times 10^{-8}\right)\)

A certain acid, HA, has a vapor density of \(5.11 \mathrm{g} / \mathrm{L}\) when in the gas phase at a temperature of \(25^{\circ} \mathrm{C}\) and a pressure of 1.00 atm. When 1.50 g of this acid is dissolved in enough water to make 100.0 mL of solution, the \(p\) H is found to be \(1.80 .\) Calculate \(K_{\mathrm{a}}\) for the acid.

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