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Chapter 4: Problem 35

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile,\(\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},(\mathbf{d}) \mathrm{Ba}(\mathrm{OH})_{2} .\)

Short Answer

Expert verified
(a) HF is an acid, existing as a mixture of molecules and ions in aqueous solution. (b) Acetonitrile (CH鈧僀N) is none of the above and exists almost entirely in molecular form in an aqueous solution. (c) NaClO鈧� is a salt, existing as ions in an aqueous solution. (d) Ba(OH)鈧� is a strong base, existing as ions in an aqueous solution.

Step by step solution

01

(a) HF

Hydrogen Fluoride (HF) is a binary compound of hydrogen and a halogen (fluorine). HF is an acid, specifically a hydrohalic acid. In an aqueous solution, it forms hydrogen ions (H+) and fluoride ions (F鈭�). Therefore, HF exists in aqueous solution as a mixture of molecules and ions.
02

(b) Acetonitrile (CH鈧僀N)

Acetonitrile (CH鈧僀N) is an organic compound which does not contain any ionizable hydrogen or hydroxide ions. It is not an acid, a base, or a salt. In an aqueous solution, it exists almost entirely in molecular form, as the interaction with water molecules is weak.
03

(c) NaClO鈧�

Sodium perchlorate (NaClO鈧�) is a compound consisting of a metal (sodium) and a nonmetal polyatomic ion (perchlorate). Thus, it is classified as a salt. In an aqueous solution, NaClO鈧� dissociates completely into sodium ions (Na鈦�) and perchlorate ions (ClO鈧勨伝), making it exist as ions in solution.
04

(d) Ba(OH)鈧�

Barium hydroxide (Ba(OH)鈧�) is a compound composed of a metal (barium) and hydroxide ions (OH鈦�). It is a strong base. In an aqueous solution, it dissociates completely into barium ions (Ba虏鈦�) and hydroxide ions (OH鈦�), so it exists as ions in aqueous solution.

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Key Concepts

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

Aqueous Solution
When we talk about an aqueous solution, we are referring to a situation where a substance is dissolved in water. Water, a universal solvent, has the remarkable ability to dissolve a wide variety of molecules, making it the medium for many chemical reactions.

In an aqueous solution, the dissolved substance can exist in different forms, depending on its chemical nature:
  • Molecular form: Some compounds, like acetonitrile (\(\mathrm{CH}_{3}\mathrm{CN}\)), do not ionize significantly in water. They remain largely as molecules because they lack ionizable groups.
  • Ionized form: Substances such as sodium perchlorate (\(\mathrm{NaClO}_{4}\)) dissociate entirely into ions. This behavior is common for salts and strong acids or bases.
  • Mixed form: Compounds like hydrogen fluoride (HF) exist as a mix of molecules and ions. Partially ionized solutions are typical for weak acids and bases.
Understanding how a substance behaves in an aqueous solution is crucial for predicting its reactivity and the type of chemical reactions it might undergo.
Molecular Ions
Molecular ions or polyatomic ions are charged species composed of two or more atoms covalently bonded. These ions play an important role in both organic and inorganic chemistry.

For instance, in the compound sodium perchlorate (\(\mathrm{NaClO}_{4}\)), the perchlorate ion (\(\mathrm{ClO}_{4}^{-}\)) is a polyatomic ion and carries a negative charge. Sodium ions (\(\mathrm{Na}^{+}\)) balance this negative charge in an aqueous solution.

To understand the behavior of molecular ions:
  • Dissolution in water: When salts containing polyatomic ions dissolve in water, the ions separate and disperse evenly, making them reactive.
  • Examples in acids and bases: Strong acids like hydrochloric acid (HCl) also ionize to release simple ions, while weaker acids, like HF, only partially release hydrogen ions.
Recognizing molecular ions and their interactions helps predict chemical behavior and reaction pathways.
Chemical Classification
Chemical classification involves categorizing substances based on their chemical characteristics and interactions. This classification helps in understanding the behavior of compounds in chemical reactions.

The primary classifications include acids, bases, and salts.
  • Acids: Acidic compounds like hydrogen fluoride (HF) release hydrogen ions (\(\mathrm{H}^{+}\)) when dissolved in water. They typically have low pH values (<7).
  • Bases: Compounds such as barium hydroxide (\(\mathrm{Ba(OH)}_{2}\)) release hydroxide ions (\(\mathrm{OH}^{-}\)) in aqueous solutions and have high pH values (>7).
  • Salts: Ionic compounds, like sodium perchlorate (\(\mathrm{NaClO}_{4}\)), result from the neutralization reaction of acids and bases. They dissolve in water to yield free cations and anions.
  • Neutral compounds: These don't fit into the acid, base, or salt categories, like acetonitrile (\(\mathrm{CH}_{3}\mathrm{CN}\)), and tend to remain unaltered when dissolved in water.
This systematic classification aids in understanding a compound's reactivity and potential chemical interactions.

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Most popular questions from this chapter

A solid sample of \(\mathrm{Zn}(\mathrm{OH})_{2}\) is added to 0.350 \(\mathrm{L}\) of 0.500 \(\mathrm{M}\) aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.500 \(\mathrm{MNaOH}\) solution, and it takes 88.5 mL of the NaOH solution to reach the equivalence point. What mass of \(\mathrm{Zn}(\mathrm{OH})_{2}\) was added to the HBr solution?

A 4.36 -g sample of an unknown alkali metal hydroxide is dissolved in 100.0 \(\mathrm{mL}\) of water. An acid-base indicator is added, and the resulting solution is titrated with 2.50 \(\mathrm{M} \mathrm{HCl}(a q)\) solution. The indicator changes color, signaling that theequivalence point has been reached, after 17.0 \(\mathrm{mL}\) of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the alkalimetal cation: \(\mathrm{Li}^{+}, \mathrm{Na}^{+}, \mathrm{K}^{+}, \mathrm{Rb}^{+},\) or \(\mathrm{Cs}^{+} ?\)

An 8.65 -g sample of an unknown group 2 A metal hydroxide is dissolved in 85.0 \(\mathrm{mL}\) of water. An acid-base indicator is added and the resulting solution is titrated with 2.50 \(\mathrm{M}\) \(\mathrm{HCl}(a q)\) solution. The indicator changes color, signaling that the equivalence point has been reached, after 56.9 \(\mathrm{mL}\) of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the metal cation: \(\mathrm{Ca}^{2+}, \mathrm{Sr}^{2+},\) or \(\mathrm{Ba}^{2+?}\) ?

Consider the following reagents: zinc, copper, mercury (density 13.6 \(\mathrm{g} / \mathrm{mL}\) , silver nitrate solution, nitric acid solution. (a) Given a 500 -mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?

Tartaric acid, \(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) , has two acidic hydrogens. The acid is often present in wines and a salt derived from the acid precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 24.65 \(\mathrm{mL}\) of 0.2500 \(\mathrm{M}\) NaOH solution to titrate both acidic protons in 50.00 \(\mathrm{mL}\) of the tartaric acid solution. Write a balanced net ionic equation for the neutralization reaction, and calculate the molarity of the tartaric acid solution.
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