Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 10

A certain sodium compound is dissolved in water to liberate Na' ions and a certain negative ion. What evidence would you look for to determine whether the anion is behaving as an acid or a base? How could you tell whether the anion is a strong base? Explain how the anion could behave simultaneously as an acid and a base.

Short Answer

Expert verified
To determine if an anion is behaving as an acid or a base, we can measure the pH of the solution and observe the reaction products. Acidic solutions will have pH less than 7, while basic solutions will have pH greater than 7. A strong base will have a high pH value, close to 14, and undergo complete ionization in water, producing a significant amount of hydroxide ions (OH-). An anion can behave simultaneously as an acid and a base if it can both donate (acid) and accept (base) protons, like an amphoteric substance such as the hydrogen carbonate ion (HCO3-).

Step by step solution

01

Identifying the behavior of the anion as an acid or a base

When a sodium compound is dissolved in water, it liberates sodium ions (Na+) and a negative ion (anion). To determine if the anion is behaving as an acid or a base, we will look at the reaction of the anion when it is dissolved in water. If the anion donates a proton (H+) to water, it behaves as an acid. If the anion accepts a proton from water, it behaves as a base.
02

Look for evidence to determine the anion's behavior

To determine whether the anion is behaving as an acid or a base, we will rely on the following evidence: 1. Measure the pH of the solution: An acidic solution (anion behaves as an acid) will have a pH less than 7, while a basic solution (anion behaves as a base) will have a pH greater than 7. 2. Look for the reaction products: If the anion donates a proton (H+) to water, forming hydronium ions (H3O+), the solution will be acidic. If the anion accepts a proton from water, forming hydroxide ions (OH-), the solution will be basic.
03

Identifying if the anion is a strong base

A strong base is a substance that readily donates hydroxide (OH-) ions when dissolved in water. To determine if the anion is a strong base, we will look for: 1. High pH value: A strong base will result in a solution with a pH value closer to 14. 2. Complete ionization: A strong base will undergo complete ionization in water, producing a significant amount of hydroxide ions (OH-). Look for the ionization reaction products and compare with the ionization reactions for strong bases.
04

Explaining how the anion could behave simultaneously as an acid and a base

An anion that can behave simultaneously as an acid and a base is called an amphoteric substance. For an anion to be amphoteric, it must be able to both donate (acid) and accept (base) protons. An example of an amphoteric anion is the hydrogen carbonate ion (HCO3-). When dissolved in water, hydrogen carbonate can both donate a proton (acting as an acid), forming carbonic acid (H2CO3) or accept a proton (acting as a base), forming carbonate ion (CO3^2-). In summary, understanding the properties and reactions of anions in aqueous solutions will allow us to determine their behavior as acids or bases, identify strong bases, and explain the potential amphoteric behavior of certain anions/hydrogen carbonate.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A \(1.0 \times 10^{-2}-M\) solution of cyanic acid (HOCN) is 17\(\%\) dissociated. Calculate \(K_{\mathrm{a}}\) for cyanic acid.

Calculate \(\left[\mathrm{OH}^{-}\right], \mathrm{pOH}\) , and pH for each of the following. a. 0.00040\(M \mathrm{Ca}(\mathrm{OH})_{2}\) b. a solution containing 25 \(\mathrm{g}\) KOH per liter c. a solution containing 150.0 \(\mathrm{g}\) NaOH per liter

Trichloroacetic acid $\left(\mathrm{CCl}_{3} \mathrm{CO}_{2} \mathrm{H}\right)$ is a corrosive acid that is used to precipitate proteins. The pH of a \(0.050-M\) solution of trichloroacetic acid is the same as the pH of a \(0.040-M \mathrm{HClO}_{4}\) solution. Calculate \(K_{\mathrm{a}}\) for trichloroacetic acid.

When determining the pH of a weak acid solution, sometimes the 5\(\%\) rule can be applied to simplify the math. At what \(K_{\mathrm{a}}\) values will a \(1.0-M\) solution of a weak acid follow the 5\(\%\) rule?

Write out the stepwise \(K_{\mathrm{a}}\) reactions for citric acid \(\left(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)\) a triprotic acid.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free