/*! 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 5 What types of substances are str... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 5

What types of substances are strong electrolytes? How do they behave when dissolved in water?

Short Answer

Expert verified
Strong electrolytes are substances like salts, strong acids, and strong bases that completely dissociate into ions when dissolved in water. They are great conductors of electricity because of the large number of ions present in the solution.

Step by step solution

01

Define Strong Electrolytes

Strong electrolytes are substances that completely dissociate into ions when they dissolve in water. Meaning, they can separate into individual cations (positively charged ions) and anions (negatively charged ions) when dissolved in water. Common examples of strong electrolytes include salts like NaCl (sodium chloride), strong acids like HCl (hydrochloric acid), and strong bases like NaOH (sodium hydroxide).
02

Explain the Dissolution of Strong Electrolytes in Water

When strong electrolytes dissolve in water, they break into their constituent cations and anions. This complete ionization in water allows these solutions to conduct electricity efficiently, because of the mobility of the ions. The more ions a solution has, the stronger its electrical conductivity. Therefore, strong electrolytes yield solutions with high conductivity.
03

Correlate the Nature of Strong Electrolytes with Their Electrical Conductivity

Since strong electrolytes fully ionize in water, there are large amounts of ions present in the solution. These ions can move freely under the influence of an electric field, which allows electrical current to pass through the solution. This is the main reason why strong electrolytes are excellent conductors of electricity in aqueous solutions.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Dissociation
When discussing strong electrolytes, the concept of dissociation is fundamental. Dissociation is the process where strong electrolytes separate into individual ions when dissolved in water. This process occurs because the ions in the compound are stabilized by the surrounding water molecules.

For example, when sodium chloride (NaCl) dissolves in water, it dissociates into sodium ions (Na+) and chloride ions (Cl-). This separation is complete, meaning that nearly all of the NaCl dissociates into its respective ions. This characteristic defines strong electrolytes.
  • Complete separation of components in water
  • Common in salts, strong acids, and bases
  • Critical for electrical conductivity
Ions
Ions are crucial to understanding how strong electrolytes work. Ions are atoms or molecules that carry an electric charge due to the loss or gain of one or more electrons.

Strong electrolytes are made up of cations (positively charged ions) and anions (negatively charged ions). In aqueous solutions, these ions move freely and are the source of the electrical conductivity of the solution.
  • Cations: Positively charged (e.g., Na+)
  • Anions: Negatively charged (e.g., Cl-)
  • Formed through complete dissociation in water
Electrical Conductivity
Electrical conductivity is a key property of solutions containing strong electrolytes. The ability of a solution to conduct electricity depends on the presence of charged particles, specifically ions, which are supplied through the dissociation process.

In solutions of strong electrolytes, the abundance of ions allows electric current to flow freely through the solution. This is because the ions move under an electric field, carrying the charge from one electrode to the other. Hence, solutions of strong electrolytes like NaCl, HCl, and NaOH have high electrical conductivity due to the high concentration of mobile ions.
  • Relies on ion mobility in solution
  • High in solutions with complete ionization
  • Essential for applications in electrochemistry
Aqueous Solutions
An aqueous solution is simply a solution where water is the solvent. For strong electrolytes, water plays a vital role by facilitating dissociation into ions.

When a strong electrolyte is placed into water, the molecules separate into their respective ions. This transformation is because water is a polar solvent, meaning it has a partial positive and negative charge which stabilizes the ions once they dissociate.
  • Water as the medium for ion formation
  • Involves interaction between water molecules and electrolytes
  • Crucial for ensuring high ion concentration in solution

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

When an ionic solid dissolves in water, which of the processes involved in the solution process require energy? Which release energy?

Iodine, \(\mathrm{I}_{2}\), is very soluble in hexane, \(\mathrm{C}_{6} \mathrm{H}_{14}\), but not in water. Explain this using the rule "like dissolves like."

Identify the solute and solvent in each of the following solutions. (a) seawater (b) steel, an alloy of iron which contains up to \(1.5 \%\) carbon (c) oxygenated water

What is the molarity of a concentrated HBr solution if the solution is \(48.0 \% \mathrm{HBr}\) by mass and has a density of \(1.50 \mathrm{~g} / \mathrm{mL}\) ?

How many moles of sodium carbonate, \(\mathrm{Na}_{2} \mathrm{CO}_{3}\), are required to precipitate the calcium ion from \(850.0 \mathrm{~mL}\) of a \(0.35 \mathrm{M} \mathrm{CaCl}_{2}\) solution? (Begin by writing a balanced chemical equation for the reaction.)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

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.