6. Chemical Quantities & Aqueous Reactions

Electrolytes

Electrolytes: Definition, Examples, & Practice

The following aqueous solutions were tested with a light bulb conductivity apparatus, as shown in Figure 4.3. What result—dark, dim, or bright—do you expect from each? 
(a) 0.10 M hydrofluoric acid 
(b) 0.10 M sodium chloride 
(c) 0.10 M glucose (C6H12O6)

Each of the following reactions depicts a solute dissolving in water. Classify each solute as a strong electrolyte, a weak electrolyte or a non-electrolyte.

How to Identify Strong, Weak, and Non-Electrolytes Examples & Practice Problems

Ionic compounds can produce positive and negative ions in solution.

Ionic compounds do contain negative and positive ions which may produce ions in solution.

Nonelectrolytes do not dissociate into ions in solution.

There are no ions formed in solution by nonelectrolytes.

A weak acid is an example of a weak electrolyte.

A weak acid only partially dissociates into ions.

At least one of the given statements is correct.

 The classifications of electrolytes depends on how the solute dissociates in solution. 

Which of the following statements is false?

Magnesium, the element, is produced commercially by
electrolysis from a molten salt (the “electrolyte”) using a
cell similar to the one shown here. (b) Chlorine gas is evolved as voltage is applied in the cell.
Knowing this, identify the electrolyte. 


<img src="https://lightcat-files.s3.amazonaws.com/problem_images/1c62a61f4cd35394-1665499626848.jpg" alt="" />

State whether each of the following statements is true or 
false. Justify your answer in each case. 
(b) If you add a nonelectrolyte to an aqueous solution that 
already contains an electrolyte, the electrical conductivity 
will not change.

Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous
acid, HClO, is a weak electrolyte; and ammonium chloride,
NH4Cl, is a strong electrolyte. (a) What are the solutes present
in aqueous solutions of each compound?
What solute particles are present in an aqueous solution of HClO?

Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous
acid, HClO, is a weak electrolyte; and ammonium chloride,
NH4Cl, is a strong electrolyte. (b) If 0.1 mol of
each compound is dissolved in solution, which one contains
0.2 mol of solute particles, which contains 0.1 mol of solute
particles, and which contains somewhere between 0.1 and
0.2 mol of solute particles?

Electrolytes Concept 3

CHEMISTRY 101 - Electrolyte and nonelectrolyte solutions

Which of the following represents a strong base?

The following aqueous solutions were tested with a light bulb conductivity apparatus, as shown in Figure 4.3. What result—dark, dim, or bright—do you expect from each? 
(a) 0.10 M potassium chloride 
(b) 0.10 M methanol 
(c) 0.10 M acetic acid<img src="https://lightcat-files.s3.amazonaws.com/problem_images/529a73c2dec0ee14-1669059116922.jpg" alt="" />

What Are Electrolytes?

Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous
acid, HClO, is a weak electrolyte; and ammonium chloride,
NH4Cl, is a strong electrolyte. (a) What are the solutes present
in aqueous solutions of each compound?
What solute particles are present in an aqueous solution of CH3COCH3?

We have learned in this chapter that many ionic solids dissolve
in water as strong electrolytes; that is, as separated
ions in solution. Which statement is most correct about
this process? (a) Water is a strong acid and therefore is good
at dissolving ionic solids. (b) Water is good at solvating ions
because the hydrogen and oxygen atoms in water molecules
bear partial charges. (c) The hydrogen and oxygen bonds of
water are easily broken by ionic solids.

Strong Electrolytes break up into ions completely and are grouped into 3 categories:Strong Acids, Strong Bases and Soluble Ionic Compounds.&#160;

Electrolytes Example 2

Categories of the Electrolytes

Why do we use a double arrow  to show the dissociation of a weak acid or weak base in aqueous solution?

When carbon dioxide dissolves in water, it is in equilibrium 
with carbonic acid H2CO3, which is a weak electrolyte. 
Write the chemical equation for the ionization of 
H2CO3.

Non-Electrolytes&#160;do NOT break up into ions at all and are commonly referred to as&#160;molecular compounds.&#160;

Classify each compound as a strong electrolyte or
nonelectrolyte.
a. MgBr2
b. C12H22O11
c. Na2CO3
d. KOH

Electrolytes Concept 4

Use the molecular representations shown here to classify
each compound as a nonelectrolyte, a weak electrolyte,
or a strong electrolyte (see Figure 4.6 for the element color
scheme).
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/c2d6e9906ef5bff4-1676503680225.jpg" alt="" />

Evaluating Electrolytes and Nonelectrolytes

For each compound (all water soluble), would you expect the
resulting aqueous solution to conduct electrical current?
a. CsCl
b. CH3OH
c. Ca(NO2)2
d. C6H12O6

Is it possible for a molecular substance to be a strong electrolyte? Explain.

Classify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte.
(a) HBr
(b) HF
(c) NaClO4 
(d) (NH4)2CO3 
(e) NH3
(f) Ethyl alcohol

Refer to the figure to answer questions 4 and 5. The images are a molecular representation of three different substances, AX3, AY3, and AZ3, dissolved in water. (Water molecules are omitted for clarity.) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/e7b92591858ca9f3-1669048527645.jpg" alt="" />
Which of the substances is the weakest electrolyte? (LO 4.6)
(a) AX3 
(b) AY3 
(c) AZ3 
(d) All of the substances are strong electrolytes.

When carbon dioxide dissolves in water, it is in equilibrium
with carbonic acid H2CO3, which is a weak electrolyte. What
solutes are present in an aqueous solution of this compound?

Perbromic acid, HBrO4, represents a weak electrolyte

Lithium chloride, LiCl, represents a non-electrolyte

Formic acid, HCO2H, represents a strong electrolyte

Zinc Bromide, ZnBr2, represents a strong electrolyte

Propanol, C3H8OH, represents a weak electrolyte

Which of the following statements is true? &nbsp;

Electrolytes Example 1

Weak Electrolytes&#160;partially break up into ions and are grouped into 2 categories:&#160;Weak Acids&#160;and&#160;Weak Bases.&#160;

Electrolytes Concept 2

sugar (C12H22O11)

Sugar does not produce ions in aqueous solution.

Correct, aqueous solutions of soluble ionic compounds conduct electricity.

Ethanol does not produce ions in aqueous solution.

Aqueous solutions of soluble ionic compounds conduct electricity.

 Solutes that produce ions in solution are known as electrolytes.  Solutions that contain electrolytes will conduct electricity.  

An aqueous solution of which of the following would conduct electricity?

Aqueous solutions of three different substances, AX, AY, and
AZ, are represented by the three accompanying diagrams.
Identify each substance as a strong electrolyte, a weak electrolyte,
or a nonelectrolyte.
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/b737edd3ef9185e6-1660652232570.jpg" alt="" />
(b) <img src="" alt="" />
(c) <img src="" alt="" />

State whether each of the following statements is true or
false. Justify your answer in each case.
(a) Electrolyte solutions conduct electricity because electrons
are moving through the solution.

Identifying Strong Electrolytes, Weak Electrolytes, and Nonelectrolytes - Chemistry Examples

Which of the following substances will produce a solution that does not conduct electricity when it dissolves in water? (LO 4.6) 
(a) NaOH
(b) HNO3 
(c) Na2SO4 
(d) CH3OH

Electrolytes Explained

(CH3)2NH2

Which of the following represents a non-electrolyte?&nbsp;

An aqueous solution of an unknown solute is tested with
litmus paper and found to be acidic. The solution is weakly
conducting compared with a solution of NaCl of the same
concentration. Which of the following substances could the
unknown be: KOH, NH3, HNO3, KClO2, H3PO3, CH3COCH3
(acetone)?

Individual solutions of Ba(OH)2 and H2SO4 both conduct electricity, but the conductivity disappears when equal molar amounts of the solutions are mixed. Explain.

Chemistry 9.2 What are Electrolytes?

A solution of HCl in water conducts electricity, but a solu-tion of HCl in chloroform, CHCl3, does not. What does this observation tell you about how HCl exists in water and how it exists in chloroform?

State whether each of the following statements is true or 
false. Justify your answer in each case. 
(b) HF is a strong acid.

Whenever you add a solute to a solvent there are three possible outcomes:the solute dissolves completely, dissolves partially or doesn&#39;t dissolve at all into ions.&#160;

Classify each of the following substances as a nonelectrolyte,
weak electrolyte, or strong electrolyte in water: (a) HF

The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z), with surrounding water mol-ecules omitted for clarity. Which of the three is the strongest acid, and which is the weakest? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/701adb2f700a998c-1668816014588.jpg" alt="" />

Assume that the electrical conductivity of a solution depends on the total concentration of dissolved ions and that you measure the conductivity of three different solutions while carrying out titration procedures: 
(a) Begin with 1.00 L of 0.100 M KCl, and titrate by adding 0.100 M AgNO3.
(b) Begin with 1.00 L of 0.100 M HF, and titrate by adding 0.100 M KOH.
(c) Begin with 1.00 L of 0.100 M BaCl2, and titrate by add-ing 0.100 M Na2SO4.
Which of the following graphs corresponds to which titration?
(1) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/06a71c5684144e9f-1670034539478.jpg" alt="" />
(2) <img src="" alt="" />
(3) <img src="" alt="" />

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1. Intro to General Chemistry

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4. BONUS: Lab Techniques and Procedures

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7. Gases

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10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

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19. Chemical Thermodynamics

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21. Nuclear Chemistry

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[BOOK CHEM] Clutch Version

Solutions

Solutions represent homogeneous mixtures made of 2 or more components that form a uniform composition.&nbsp;

Osmolarity

Osmolarity (ionic molarity) represents the number of moles of ions per liter of solution.&nbsp;

Gas Evolution Equations

A Gas Evolution Equation is a molecular equation that involves the creation of specific gases.&nbsp;

Molecular Equations

Molecular Equations show reacting molecules involved in a chemical reaction.&nbsp;

Complete Ionic Equations

Complete Ionic Equations show aqueous compounds as fully dissociated ions.&nbsp;

Solubility Rules

The Solubility Rules are a convenient set of guidelines to help us determine if a compound will be soluble or insoluble.

Molarity

Ever wonder how a mass amount such as moles can be converted into the volume amount of liters? Well, molarity serves as the bridge between moles and liters.&nbsp;

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.&nbsp;

Solution Stoichiometry

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Calculate Oxidation Numbers

Calculating Oxidation Numbers is the first pivotal step in understanding redox reactions.&nbsp;

Dilutions

In Dilutions, a solvent (usually water) is added to a concentrated solution.&nbsp;

Redox Reactions

Redox Reactions (oxidation-reduction reactions) involve transference of an electron(s) between reactants.

Activity Series

Activity Series is a list of single displacement reactions in order of reactivity.

Balancing Redox Reactions: Acidic Solutions

Balancing Redox Reactions requires a new approach that accounts for the transfer of electrons between reactants.

Balancing Redox Reactions: Basic Solutions

Balancing Basic Redox Reactions requires all the same steps as balancing in an acidic solution plus an additional step.