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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

Classify the reactions represented by the following unbalanced equations by as many methods as possible. Balance the equations. a. \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{HCl}(a q)+\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \rightarrow\) \(\mathrm{AgCl}(s)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) c. \(\mathrm{HCl}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) e. \(\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

Without first writing a full molecular or ionic equation, write the net ionic equations for any precipitation reactions that occur when aqueous solutions of the following compounds are mixed. If no reaction occurs, so indicate. a. iron(III) nitrate and sodium carbonate b. mercurous nitrate and sodium chloride c. sodium nitrate and ruthenium nitrate d. copper(II) sulfate and sodium sulfide e. lithium chloride and lead(II) nitrate f. calcium nitrate and lithium carbonate g. gold(III) chloride and sodium hydroxide

When two solutions of ionic substances are mixed and a precipitate forms, what is the net charge of the precipitate? Why?

The procedures and principles of qualitative analysis are covered in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.

By now, you are familiar with enough chemical compounds to begin to write your own chemical reaction equations. Write two examples each of what we mean by a synthesis reaction and by a decomposition reaction.
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