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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 (HClO鈧�) and nitric acid (HNO鈧�) are H鈦� and their corresponding anions, ClO鈧勨伝 and NO鈧冣伝, 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 H鈧僌鈦� ions formed#

Our given initial concentration of HClO鈧� is 0.250 M. Since the acid dissociates completely, the concentration of H鈦� ions formed in the solution will be equal to that of the HClO鈧�, 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鈦篯 is the concentration of H+ ions in the solution. Now, substitute the value of [H鈦篯 in the formula: \[ \mathrm{pH} = -\log(0.250) \] Use a calculator to find the pH: \[ \mathrm{pH} \approx 0.60 \] b. HNO鈧� #Step 1: Write the dissociation equation of HNO鈧�#

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 H鈧僌鈦� ions formed#
03

Given initial concentration of HNO鈧� is 0.250 M. Once again, the concentration of H鈦� 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鈦篯 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 HClO鈧� and 0.250 M HNO鈧� solutions is approximately 0.60.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Strong Acids
Strong acids play a crucial role in chemistry due to their unique characteristics. A strong acid is defined as an acid that completely dissociates in water. This means when you dissolve it in water, it fully separates into its constituent ions. Consider it like breaking apart a LEGO structure completely, where nothing is left attached.
For example, when you dissolve perchloric acid ( HClO鈧�) in water, it dissociates completely to form hydrogen ions ( H鈦�) and perchlorate ions ( ClO鈧勨伝). The term "strong acid" indicates that such dissociation occurs at 100% efficiency.
  • Complete dissociation increases the concentration of hydrogen ions in a solution.
  • This leads to a lower pH value, typically less than 3 for strong acids.
Understanding strong acids is key to calculating pH accurately and predicting reaction behavior in solutions.
The Process of Dissociation
Dissociation refers to the process where molecules split into smaller particles, ions in particular, when mixed with a solvent like water. In strong acids, this process is straightforward and complete.
For instance, analyzing the dissociation of perchloric acid (HClO鈧�), the reaction looks like this: \[ \mathrm{HClO}_{4} \rightarrow \mathrm{H}^{+} + \mathrm{ClO}_{4}^{-} \]
  • This formula shows that for every molecule of HClO鈧�, we get one H鈦� ion and one ClO鈧勨伝 ion.
  • The same principle applies to nitric acid (HNO鈧�) which dissociates to form H鈦� and NO鈧冣伝 ions.
Complete dissociation is what gives strong acids their potent characteristics, heavily influencing the pH of solutions.
Exploring Perchloric Acid and its Properties
Perchloric acid, with the chemical formula HClO鈧�, is one of the strongest acids known. It is highly soluble in water and dissociates completely into hydrogen ions ( H鈦�) and perchlorate ions ( ClO鈧勨伝).
When working with perchloric acid, it is essential to remember:
  • It is clear and colorless, like water.
  • Because of its complete dissociation, solutions of HClO鈧� have very low pH values.
  • Handling HClO鈧� requires caution due to its high reactivity and potential explosiveness when mixed with organic materials.
Knowing these properties is crucial for safely using perchloric acid in labs and understanding its chemical behavior.
Understanding Nitric Acid
Nitric acid ( HNO鈧�) is another strong acid that finds common use in laboratories due to its widespread applicability. Like perchloric acid, nitric acid fully dissociates in water into hydrogen ions ( H鈦�) and nitrate ions ( NO鈧冣伝).
A few essential points to remember about nitric acid:
  • HNO鈧� appears as a colorless liquid that can turn yellow over time due to decomposition.
  • It is used to manufacture fertilizers, and explosives, and in various industrial processes.
  • Its strong oxidizing properties make it useful in etching and cleaning metals.
Understanding HNO鈧冣�檚 dissociation and characteristics helps you comprehend its role in both chemical reactions and practical applications.

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Most popular questions from this chapter

Classify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous solution. a. \(\mathrm{HNO}_{2}\) b. \(\mathrm{HNO}_{3}\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) d. \(\mathrm{NaOH}\) e. \(\mathrm{NH}_{3}\) f. HF g. h. \(\mathrm{Ca}(\mathrm{OH})_{2}\) i. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

A codeine-containing cough syrup lists codeine sulfate as a major ingredient instead of codeine. The Merck Index gives \(\mathrm{C}_{36} \mathrm{H}_{44} \mathrm{N}_{2} \mathrm{O}_{10} \mathrm{S}\) as the formula for codeine sulfate. Describe the composition of codeine sulfate. (See Exercise \(155 .\) ) Why is codeine sulfate used instead of codeine?

Calculate the concentration of an aqueous \(\operatorname{Sr}(\mathrm{OH})_{2}\) that has \(\mathrm{pH}=10.50\)

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. \(\mathrm{Li}_{2} \mathrm{O}\) b. \(\mathrm{CO}_{2}\) c. SrO

A solution of formic acid (HCOOH, \(K_{\mathrm{a}}=1.8 \times 10^{-4}\) ) has a pH of \(2.70 .\) Calculate the initial concentration of formic acid in this solution.
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