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Chapter 15: Problem 53

The compound \(\mathrm{NaCl}\) is an electrolyte. (a) Is it incorrect to call \(\mathrm{NaCl}\) a molecular compound? Explain. (b) Why is \(\mathrm{NaCl}\) expected to be an electrolyte?

Short Answer

Expert verified
(a) Yes, it is incorrect to call \(\mathrm{NaCl}\) a molecular compound because it is an ionic compound formed through the transfer of electrons between sodium (Na) and chlorine (Cl), resulting in an ionic bond, not a covalent bond. (b) \(\mathrm{NaCl}\) is expected to be an electrolyte because, when dissolved in water or melted, the ionic bonds break, forming free-moving Na+ and Cl- ions in the solution. These ions can conduct electricity, making the solution conductive.

Step by step solution

01

Understanding Molecular Compounds and Electrolytes

A molecular compound consists of molecules formed by atoms bonded together through covalent bonds. These compounds have a distinct chemical formula, represented by molecules containing a fixed number of atoms. Examples of molecular compounds include \(\mathrm{H_2O}\) (water) and \(\mathrm{CO_2}\) (carbon dioxide). On the other hand, an electrolyte is a substance that conducts electricity when dissolved in water or melted. It consists of ions, which are charged particles that can freely move in solution. Electrolyte substances are typically ionic compounds and are formed through the transfer of electrons between atoms (ionic bonds). (a)
02

Determining if NaCl is a Molecular Compound

Now that we understand what molecular compounds are, let's check if \(\mathrm{NaCl}\) is a molecular compound or not. \(\mathrm{NaCl}\) is formed from sodium (Na), a metal, and chlorine (Cl), a non-metal. In this compound, sodium loses one electron and becomes positively charged (Na+) while chlorine gains one electron and becomes negatively charged (Cl-). This transfer of electrons results in an ionic bond between the two ions, forming the ionic compound \(\mathrm{NaCl}\). Since \(\mathrm{NaCl}\) is an ionic compound and not composed of molecules with covalent bonds, it is incorrect to call it a molecular compound. (b)
03

Explaining Why NaCl is an Electrolyte

To understand why \(\mathrm{NaCl}\) is expected to be an electrolyte, we need to look at its structure and properties in an aqueous solution or in its molten state. When \(\mathrm{NaCl}\) is dissolved in water or melted, the ionic bonds between the sodium (Na+) and chloride (Cl-) ions are broken. This leads to the formation of free-moving ions in the solution. These free ions in the solution are capable of carrying an electric charge, making the solution conductive. Because the ions can conduct electricity in a solution or molten state, \(\mathrm{NaCl}\) is classified as an electrolyte.

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Most popular questions from this chapter

The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?

\(\mathrm{HZ}\) is a weak acid. An aqueous solution of \(\mathrm{HZ}\) is prepared by dissolving \(0.020\) mol of \(\mathrm{HZ}\) in sufficient water to yield \(1.0 \mathrm{~L}\) of solution. The \(\mathrm{pH}\) of the solution was \(4.93\) at \(25.0{ }^{\circ} \mathrm{C}\). What is the \(K_{\mathrm{a}}\) of \(\mathrm{HZ}\) ?

Citric acid, \(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\), is a weak triprotic acid. Write equations for the three equilibrium reactions that occur during the stepwise dissociation of citric acid in water.

Why is a pH of 7 equal to neutrality?

Complete the following sentence: "The lower the \(\mathrm{p} K_{\mathrm{a}}\), the (stronger/weaker) the acid." \(^{\prime \prime}\) How does this parallel pH?
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