/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 7 What is meant by a strong electr... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Balance each of the following equations that describe combustion reactions. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{C}_{4} \mathrm{H}_{10}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) c. \(C_{6} \mathrm{H}_{14}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

Balance each of the following equations that describe decomposition reactions. a. \(\mathrm{NaHCO}_{3}(s) \rightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g)\) b. \(\mathrm{NaClO}_{3}(s) \rightarrow \mathrm{NaCl}(s)+\mathrm{O}_{2}(g)\) c. \(\mathrm{HgO}(s) \rightarrow \mathrm{Hg}(l)+\mathrm{O}_{2}(g)\) d. \(C_{12} H_{22} O_{11}(s) \rightarrow C(s)+H_{2} O(g)\) e. \(\mathrm{H}_{2} \mathrm{O}_{2}(l) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\)

Describe briefly what happens when an ionic substance is dissolved in water.

Balance each of the following equations that describe synthesis reactions. a. \(\operatorname{Co}(s)+S(s) \rightarrow C o_{2} S_{3}(s)\) b. \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}_{2}(g)\) c. \(\mathrm{FeO}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{FeCO}_{3}(s)\) d. \(\mathrm{Al}(s)+\mathrm{F}_{2}(g) \rightarrow \mathrm{AlF}_{3}(s)\) e. \(\mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(s)\)

For each of the following unbalanced molecular equations, write the corresponding balanced net ionic equation for the reaction. a. \(\mathrm{HCl}(a q)+\mathrm{AgNO}_{3}(a q) \rightarrow \mathrm{AgCl}(s)+\mathrm{HNO}_{3}(a q)\) b. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{3} \mathrm{PO}_{4}(a q) \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\) \(\mathrm{NaCl}(a q)\) c. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{BaCl}_{2}(a q) \rightarrow\) \(\mathrm{PbCl}_{2}(s)+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) d. \(\operatorname{FeCl}_{3}(a q)+\operatorname{NaOH}(a q) \rightarrow \operatorname{Fe}(\mathrm{OH})_{3}(s)+\mathrm{NaCl}(a q)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.