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Chapter 7: Problem 7

What is meant by a strong electrolyte? Give two examples of substances that behave in solution as strong electrolytes.

Short Answer

Expert verified
A strong electrolyte is a solute that completely dissociates into its constituent ions in a solution, allowing it to conduct electric current effectively. Examples of strong electrolytes include salts, strong acids, and strong bases. Two common examples of strong electrolytes are sodium chloride (NaCl) and hydrochloric acid (HCl). Sodium chloride is an ionic compound that dissolves completely in water, forming positive sodium ions (Na+) and negative chloride ions (Cl-). Hydrochloric acid is a strong acid that dissociates completely in water, forming positive hydrogen ions (H+) and negative chloride ions (Cl-). Both substances exhibit high electrical conductivity in their solutions due to their complete dissociation.

Step by step solution

01

Defining strong electrolyte

A strong electrolyte is a solute that completely dissociates into its constituent ions in a solution, which allows the solution to conduct an electric current effectively. This means that, when a strong electrolyte is dissolved in a solvent like water, there are no remaining molecules of the electrolyte, only the dissociated ions. Examples of strong electrolytes include salts, strong acids, and strong bases.
02

Providing examples of strong electrolytes

Two common examples of strong electrolytes are: 1. Sodium chloride (NaCl): Sodium chloride is an ionic compound that dissolves completely in water, resulting in a solution containing positive sodium ions (Na+) and negative chloride ions (Cl-). The complete dissociation of NaCl into its ions allows the solution to conduct electricity effectively. 2. Hydrochloric acid (HCl): Hydrochloric acid is a strong acid that dissociates completely in water, forming positive hydrogen ions (H+) and negative chloride ions (Cl-). The complete dissociation of HCl results in a highly conductive solution with a high concentration of ions. These examples show substances that, when dissolved in water, dissociate completely into their constituent ions and exhibit high electrical conductivity in the solution.

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Most popular questions from this chapter

Balance each of the following oxidation-reduction reactions. In each, indicate which substance is being oxidized and which is being reduced. a. \(\mathrm{Na}(s)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{S}(s)\) b. \(\operatorname{Mg}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{MgO}(s)\) c. \(\mathrm{Ca}(s)+\mathrm{F}_{2}(g) \rightarrow \mathrm{CaF}_{2}(s)\) d. \(\operatorname{Fe}(s)+\mathrm{Cl}_{2}(g) \rightarrow \operatorname{Fe} \mathrm{Cl}_{3}(s)\)

There is much overlapping of the classification schemes for reactions discussed in this chapter. Give an example of a reaction that is, at the same time,an oxidation-reduction reaction, a combustion reaction, and a synthesis reaction.

Sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), oxidizes many metallic elements. One of the effects of acid rain is that it produces sulfuric acid in the atmosphere, which then reacts with metals used in construction. Write balanced oxidation-reduction equations for the reaction of sulfuric acid with Fe, \(\mathrm{Zn}, \mathrm{Mg}, \mathrm{Co},\) and \(\mathrm{Ni}\).

What is a synthesis or combination reaction? Give an example. Can such reactions also be classified in other ways? Give an example of a synthesis reaction that is also a combustion reaction. Give an example of a synthesis reaction that is also an oxidation-reduction reaction, but which does not involve combustion.

For the reaction \(\mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s),\) illustrate how electrons are gained and lost during the reaction.
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