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Chapter 7: Problem 31

What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain.

Short Answer

Expert verified
A strong acid is a substance that completely ionizes or dissociates into its constituent ions (H+ and anions) when dissolved in water, such as HCl, HNO₃, and H₂SO₄. Strong acids are considered strong electrolytes since their complete ionization produces a high concentration of freely moving ions, which facilitates the conduction of electrical current in aqueous solutions.

Step by step solution

01

Definition of Strong Acids

A strong acid is a substance that completely ionizes or dissociates into its constituent ions when dissolved in water. In other words, a strong acid loses its protons (H+) when dissolved in water, producing a high concentration of H+ ions and its corresponding anions. Some examples of strong acids include hydrochloric acid (HCl), nitric acid (HNO₃), and sulfuric acid (H₂SO₄).
02

The Relationship Between Strong Acids and Strong Electrolytes

Strong acids are categorized as strong electrolytes because they are excellent conductors of electricity when dissolved in water. The reason for this is that the complete ionization/dissociation of strong acids in water results in a significant number of freely moving ions within the solution, which facilitates the conduction of electrical current.
03

Explanation of the Relationship Between Strong Acids and Strong Electrolytes

The electrical conductivity in a solution depends on the amount of charge-carrying ions present in the solution. Since strong acids completely ionize by releasing H+ ions and their corresponding anions when dissolved in water, they produce a high concentration of ions that can move freely and participate in the conduction of electricity. Therefore, strong acids are considered strong electrolytes because their complete ionization results in a greater ability to conduct electricity in aqueous solutions.

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Most popular questions from this chapter

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.

Although the metals of Group 2 of the periodic table are not nearly as reactive as those of Group \(1,\) many of the Group 2 metals will combine with common nonmetals, especially at elevated temperatures. Write balanced chemical equations for the reactions of \(\mathrm{Mg}\) \(\mathrm{Ca}, \mathrm{Sr},\) and \(\mathrm{Ba}\) with \(\mathrm{Cl}_{2}, \mathrm{Br}_{2},\) and \(\mathrm{O}_{2}\).

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. \(\operatorname{Fe}(s)+\mathrm{Cl}_{2}(g) \rightarrow \operatorname{Fe} \mathrm{Cl}_{3}(s)\)

Corrosion of metals costs us billions of dollars annually, slowly destroying cars, bridges, and buildings. Corrosion of a metal involves the oxidation of the metal by the oxygen in the air, typically in the presence of moisture. Write a balanced equation for the reaction of each of the following metals with \(\mathrm{O}_{2}: \mathrm{Zn}\) \(\mathrm{Al}, \mathrm{Fe}, \mathrm{Cr},\) and \(\mathrm{Ni}\).

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid-base, or oxidation-reduction. a. \(\operatorname{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Fe}_{3}\left(\mathrm{SO}_{4}\right)_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{HClO}_{4}(a q)+\mathrm{RbOH}(a q) \rightarrow \mathrm{RbClO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) \(\overline{\mathrm{c}} . \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CaO}(s)\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) e. \(\operatorname{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow\) \(\mathrm{PbCO}_{3}(s)+\mathrm{NaNO}_{3}(a q)\) f. \(\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{KCl}(a q)+\mathrm{CaSO}_{4}(s)\) g. \(\mathrm{HNO}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{KNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) h. \(\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{S}(a q) \rightarrow\) \(\mathrm{NiS}(s)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) i. \(\mathrm{Ni}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{NiCl}_{2}(s)\)
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