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Chapter 15: Problem 46

Hydrogen chloride and water are molecular compounds, yet a solution of HCl dissolved in \(\mathrm{H}_{2} \mathrm{O}\) is an excellent conductor of electricity. Explain why.

Short Answer

Expert verified
A solution of hydrogen chloride (HCl) dissolved in water is an excellent conductor of electricity because of the ionization process that occurs when HCl dissolves in water. This process results in the formation of positively charged hydronium ions (H鈧僌鈦�) and negatively charged chloride ions (Cl鈦�), which can move freely through the solution and carry electric charges. Although HCl is a molecular compound, its interaction with water leads to ion formation, enabling the resulting solution to conduct electricity efficiently.

Step by step solution

01

Molecular compounds are formed by the sharing of electrons between non-metal atoms, resulting in the formation of covalent bonds. Unlike ionic compounds, they do not generally dissociate into ions when dissolved in water. As a result, they typically do not conduct electricity when dissolved in water, as there are no ions to carry the electric charge. #Step 2: Hydrogen chloride (HCl) in water#

HCl is a molecular compound, but when it dissolves in water, there is a strong interaction between the hydrogen and chlorine atoms of HCl and the oxygen and hydrogen atoms of water molecules. This interaction results in the so-called ionization of HCl, whereby HCl molecules break apart and form ions in the solution. #Step 3: Ionization of HCl in water#
02

The ionization of HCl in water produces two types of ions: (1) positively charged hydrogen ions (protons) represented as \(\mathrm{H}^{+}\), and (2) negatively charged chloride ions, represented as \(\mathrm{Cl}^{鈥搣\). The ionization of HCl in water can be presented by the following equation: HCl + H\(_2\)O \(\longrightarrow\) H\(_3\)O\(^+\) + Cl\(^-\) The reaction shows the transfer of proton (H\(^+\)) from HCl to a water molecule, forming hydronium ion (H\(_3\)O\(^+\)) and chloride ion (Cl\(^-\)) in the solution. #Step 4: Conductivity of HCl solution#

As HCl dissolves in water and ionizes to form positively charged hydronium ions and negatively charged chloride ions, it creates a solution with a high concentration of mobile charge carriers. These ions can move freely through the solution, allowing electric charges to be transferred from one point to another. This results in the HCl solution being an excellent conductor of electricity. In conclusion, the reason why an HCl solution in water is an excellent conductor of electricity is the ionization process that occurs when HCl dissolves in water, producing a significant amount of ions that can carry electric charges through the solution. Even though HCl is a molecular compound, its interaction with water leads to ion formation, which enables the resulting solution to conduct electricity efficiently.

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Most popular questions from this chapter

Neutralizing the Smell of Fish Trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}\) \(\left(K_{\mathrm{b}}=6.5 \times 10^{-5} \text {at } 25^{\circ} \mathrm{C}\right),\) contributes to the "fishy" odor of not-so-fresh seafood. Some people squeeze fresh lemon juice (which contains a high concentration of citric acid) on cooked fish to reduce the fishy odor. Why is this practice effective?

Predict which solution in each pair below will have the lower pH. a. \(2.56 \times 10^{-2} \mathrm{M} \mathrm{HCl}\) or \(4.09 \times 10^{-2} \mathrm{MHBr}\) b. \(1.00 \times 10^{-5} M\) acctic acid \(\left(K_{\mathrm{a}}=1.76 \times 10^{-5}\right)\) or \(1.00 \times 10^{-5} M\) formic acid \(\left(K_{a}=1.77 \times 10^{-4}\right)\) c. \(22 \mathrm{mM} \mathrm{CH}_{3} \mathrm{NH}_{2}\left(\mathrm{p} K_{\mathrm{b}}=3.36\right)\) or \(22 \mathrm{mM}\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\left(K_{\mathrm{b}}=5.9 \times 10^{-4}\right)\) d. \(158 \mathrm{mM} \mathrm{NH}_{3}\left(\mathrm{p} K_{\mathrm{b}}=4.75\right)\) or \(158 \mathrm{m} M\) acetic acid \(\left(p K_{a}=4.75\right)\) e. \(0.00395 M \mathrm{HNO}_{3}\) or \(0.00145 M \mathrm{HClO}_{4}\) f. \(2.05 \times 10^{-1} M\) propionic acid \(\left(K_{2}=1.4 \times 10^{-5}\right)\) or \(2.05 \times 10^{-1} M\) fluoroacetic acid \(\left(K_{2}=2.6 \times 10^{-3}\right)\) g. 375 m \(M\) pyridine \(\left(p K_{b}=8.77\right)\) or \(375 \mathrm{mM}\) aniline \(\left(\mathrm{p} K_{\mathrm{b}}=9.40\right)\) h. \(0.555 M \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\left(K_{2}=3 \times 10^{-3}\right)\) or \(0.355 M \mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}\left(K_{2}=1 \times 10^{-4}\right)\)

Why is it unnecessary to publish tables of \(K_{\mathrm{b}}\) values of the conjugate bases of weak acids whose \(K_{\mathrm{a}}\) values are known?

What is the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions in \(0.65 \mathrm{M} \mathrm{HNO}_{3} ?\)

Liquid ammonia at a temperature of 223 K undergoes autoionization. The value of the equilibrium constant for the autoionization of ammonia is considerably less than that of water. Write an equation for the autoionization of ammonia and suggest a reason why the value of \(K\) for the process is less than that of water.
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