6. Chemical Quantities & Aqueous Reactions

Electrolytes

6. Chemical Quantities & Aqueous Reactions

Electrolytes

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Categories of the Electrolytes

Electrolytes Example 1

Electrolytes Concept 2

Electrolytes Concept 3

Electrolytes Example 2

Electrolytes Concept 4

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07:48

What Are Electrolytes?

Professor Dave Explains

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Evaluating Electrolytes and Nonelectrolytes

01:03

Evaluating Electrolytes and Nonelectrolytes

CHEMISTRY 101 - Electrolyte and nonelectrolyte solutions

Chemistry 9.2 What are Electrolytes?

Electrolytes Explained

Electrolytes: Definition, Examples, & Practice

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

The Organic Chemistry Tutor

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

05:44

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

Conquer Chemistry

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Multiple Choice

Which of the following represents a strong base?

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Multiple Choice

Which of the following represents a non-electrolyte?

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Multiple Choice

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.

a) PbSO₄ (s) → PbSO₄ (aq)

b) HC₂H₃O₂ (aq) ⇌ H⁺ (aq) + C₂H₃O₂⁻ (aq)

c) CaS (s) → Ca²⁺ (aq) + S²⁻ (aq)

d) Hg (l) → Hg (aq)

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Multiple Choice

Which of the following statements is true?

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Multiple Choice

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

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Multiple Choice

Which of the following statements is false?

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Textbook Question

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)

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Textbook Question

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)

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Textbook Question

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.)

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.

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Textbook Question

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

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Textbook Question

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.

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Textbook Question

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.

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Textbook Question

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.

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Textbook Question

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.

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Textbook Question

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.

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Textbook Question

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?

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Textbook Question

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?

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Textbook Question

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?

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Textbook Question

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Textbook Question

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

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Textbook Question

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)?

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Textbook Question

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

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Textbook Question

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?

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Textbook Question

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)

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Textbook Question

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

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Textbook Question

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)

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Textbook Question

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.

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Textbook Question

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?

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Open Question

Which substance will most likely ionize when it is dissolved in water: HBr, CaBr₂, MgCl₂, or KCl?

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Open Question

How does a conductivity apparatus test whether a solution has ionic or covalent substances in it?

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Open Question

Which substance will most likely dissociate when it is dissolved in water? NO₂, N₂F₆, CaCl₂, C₆H₁₂O₆

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Open Question

Which compound will conduct electricity when it is dissolved in water? CH₄, CuSO₄, C₆H₆, C₆H₁₂O₆.

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Open Question

Which of these salts is the best electrolyte?

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Open Question

Which two compounds are electrolytes?

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Open Question

What solute particles are present in an aqueous solution of HClO?

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Open Question

Each of the following compounds is soluble in water. for which compounds do you expect the resulting aqueous solution to conduct electrical current?

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Open Question

Classify each of the following as a strong electrolyte or nonelectrolyte.

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Open Question

Of the species below, only ________ is not an electrolyte.

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Open Question

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water.

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Open Question

Which of the following is an electrolyte

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Open Question

Which of the following is true of electrolytes

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Open Question

A substance is classified as an electrolyte because

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Open Question

Which substance is an electrolyte?

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Open Question

A substance that carries an electric current when dissolved in water is called a(n)

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Open Question

What is the best reason for the difference in properties of LiCl and C₆H₁₄O?

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Open Question

A substance that ionizes or dissociates into ions when placed in water is always a

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Open Question

Which compound will conduct electricity when it is dissolved in water? CH₄ CuSO₄ C₆H₆ C₆H₁₂O₆

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Open Question

The second test is for solubility. If the substance is soluble in water, then it is likely

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Open Question

Determine whether each of the given characteristics refers to electrolytes or non-electrolytes.

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Open Question

Determine whether each of the given characteristics refers to electrolytes or non-electrolytes.

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Open Question

Which symbol in a chemical equation separates the reactants from the products?=→>+

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Open Question

A 0.12 M solution of an acid that ionizes only slightly in solution would be termed _____.

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Open Question

Table salt is considered a(n) ______________ because it conducts electricity in water.

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Open Question

Which of the compounds below will ionize in water? Check all that apply. HSO NH NaCl SO MgBr

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6. Chemical Quantities & Aqueous Reactions

Electrolytes

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