/*! 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 37 Classify each of the following s... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 37

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) \(\mathrm{H}_{2} \mathrm{SO}_{3}\) , (b) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (ethanol), \((\mathbf{c}) \mathrm{NH}_{3},(\mathbf{d}) \mathrm{KClO}_{3}\), \((\mathbf{e}) \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\).

Short Answer

Expert verified
In summary: a) \(H_2SO_3\) - weak electrolyte b) \(CH_3CH_2OH\) (Ethanol) - nonelectrolyte c) \(NH_3\) - weak electrolyte d) \(KClO_3\) - strong electrolyte e) \(Cu(NO_3)_2\) - strong electrolyte

Step by step solution

01

Classifying H2SO3

Sulfurous acid (H2SO3) is a weak acid, which means it will partially ionize in water. Thus, H2SO3 is a weak electrolyte.
02

Classifying CH3CH2OH (Ethanol)

Ethanol (CH3CH2OH) is an organic compound that is soluble in water but does not dissociate into ions. Therefore, ethanol is a nonelectrolyte.
03

Classifying NH3 (Ammonia)

Ammonia (NH3) is a weak base that partially ionizes in water to form hydroxide ions (OH-) and ammonium ions (NH4+). Since it does not ionize completely, NH3 is a weak electrolyte.
04

Classifying KClO3 (Potassium Chlorate)

Potassium Chlorate (KClO3) is an ionic compound that completely dissociates into potassium (K+) and chlorate ions (ClO3-) when dissolved in water. As a result, KClO3 is a strong electrolyte.
05

Classifying Cu(NO3)2 (Copper(II) Nitrate)

Copper(II) Nitrate (Cu(NO3)2) is an ionic compound that fully dissociates into copper (Cu2+) and nitrate ions (NO3-) when dissolved in water. This makes Cu(NO3)2 a strong electrolyte. #Summary#: In summary, the given substances can be classified into nonelectrolytes, weak electrolytes, or strong electrolytes as follows: a) H2SO3 - weak electrolyte b) CH3CH2OH (Ethanol) - nonelectrolyte c) NH3 - weak electrolyte d) KClO3 - strong electrolyte e) Cu(NO3)2 - strong electrolyte

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.

Nonelectrolyte
A nonelectrolyte is a substance that does not produce ions when dissolved in water. Consequently, it does not conduct electricity. An example of this is ethanol ((CH3CH2OH)), an organic compound with polar molecules that dissolve in water but maintain their molecular integrity without generating ions. In the classroom, students can visualize nonelectrolytes by imagining the substance dissolving like sugar or urea in water; they spread out but do not break into charged particles.
Weak Electrolyte
A weak electrolyte is a substance that only partially dissociates into ions when dissolved in water. As a result, it conducts electricity, but not as well as a strong electrolyte. Sulfurous acid (H2SO3) and ammonia (NH3) are typical examples of weak electrolytes. They create an equilibrium state where both the undissociated molecule and the ions coexist in solution. For learners, it's helpful to think of weak electrolytes as having a modest split personality鈥攑art of it breaks up into ions, while part stays intact.
Strong Electrolyte
A strong electrolyte, on the other hand, completely disassociates into ions in water. This means that it is an excellent conductor of electricity. Examples from our exercise include potassium chlorate (KClO3) and copper(II) nitrate (Cu(NO3)2). These ionic compounds break apart into their constituent ions when dissolved, resulting in a solution that contains no original molecular entities. Students can imagine this as dropping a cube of salt into water where it fragments completely into sodium and chloride ions.
Ionic Compounds
Ionic compounds are made up of positively and negatively charged ions held together by strong electrostatic forces known as ionic bonds. In the context of solubility, when these compounds are introduced to water, they typically disintegrate into their respective ions. This property is what renders substances such as KClO3 and Cu(NO3)2 strong electrolytes. The educational key here is that the complete dissociation of an ionic compound in water is synonymous with the substance being a strong electrolyte.
Dissociation in Water
Dissociation in water is a process in which ionic compounds separate into ions when they are dissolved in water. This can vary from a full separation in strong electrolytes to a partial separation in weak electrolytes. The extent and nature of this dissociation process are what determine whether a solution will conduct electricity well, poorly, or not at all. In teaching, this can be illustrated by showing animations or conducting experiments that visually demonstrate how different substances behave when dissolved in water.

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

The metal cadmium tends to form \(\mathrm{Cd}^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in \(\mathrm{CdCl}_{2}(a q),\) cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q),\) nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations. (b) Which elements more closely define the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

In each of the following pairs, indicate which has the higher concentration of \(\mathrm{I}^{-}\) ion: (a) 0.10 \(\mathrm{M}\) BaI \(_{2}\) or 0.25 \(\mathrm{M}\) KI solution, (b) 100 \(\mathrm{mL}\) of 0.10 \(\mathrm{M}\) KI solution or 200 \(\mathrm{mL}\) of 0.040 \(\mathrm{MZnI}_{2}\) solution, \((\mathbf{c}) 3.2 \mathrm{M}\) HI solution or a solution made by dissolving 145 g of Nal in water to make 150 \(\mathrm{mL}\) of solution.

Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and \(\mathrm{AgNO}_{3},\) (b) \(\mathrm{NaNO}_{3,}\) and \(\mathrm{NiSO}_{4,}\) (c) \(\mathrm{FeSO}_{4}\) and \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}.\)

Federal regulations set an upper limit of 50 parts per million \((\mathrm{ppm})\) of \(\mathrm{NH}_{3}\) in the air in a work environment \([\mathrm{that}\) is, 50 molecules of \(\mathrm{NH}_{3}(g)\) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing \(1.00 \times 10^{2} \mathrm{mL}\) of 0.0105 \(\mathrm{M}\) HCl. The \(\mathrm{NH}_{3}\) reacts with HCl according to: $$\mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q)$$ After drawing air through the acid solution for 10.0 min at a rate of 10.0 \(\mathrm{L} / \mathrm{min}\) , the acid was titrated. The remaining acid needed 13.1 \(\mathrm{mL}\) of 0.0588 \(\mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. (a) How many grams of \(\mathrm{NH}_{3}\) were drawn into the acid solution? (b) How many ppm of \(\mathrm{NH}_{3}\) were in the air? (Air has a density of 1.20 g/L and an average molar mass of 29.0 \(\mathrm{g} / \mathrm{mol}\) under the conditions of the experiment.) (c) Is this manufacturer in compliance with regulations?

Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a netionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Kinetics

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.