Textbook Question
What volume of a 2.00 M stock solution of NaOH is required to prepare 50.0 mL of 0.400 M NaOH? (LO 4.4)(a) 15.0 mL(b) 1.00 mL(c) 10.0 mL(d) 4.00 mL
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Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 6
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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Identify the nature of each substance: Determine if each substance is an electrolyte or a non-electrolyte.
Understand electrolytes: Electrolytes are substances that dissociate into ions in solution, allowing the solution to conduct electricity.
Analyze each option: (a) NaOH is a strong base and dissociates completely into Na+ and OH- ions. (b) HNO3 is a strong acid and dissociates completely into H+ and NO3- ions. (c) Na2SO4 is a salt and dissociates into 2 Na+ and SO4^2- ions.
Consider non-electrolytes: Non-electrolytes do not dissociate into ions in solution and therefore do not conduct electricity.
Evaluate option (d) CH3OH: Methanol (CH3OH) is a molecular compound that does not dissociate into ions in water, making it a non-electrolyte.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electrolytes
Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes, like NaOH and HNO3, completely ionize in solution, while weak electrolytes partially ionize. Understanding the nature of electrolytes is crucial for predicting whether a solution will conduct electricity.
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02:50
Electrolytes and Strong Acids
Non-electrolytes
Non-electrolytes are substances that do not dissociate into ions in solution and therefore do not conduct electricity. An example is CH3OH (methanol), which dissolves in water but remains as neutral molecules. Recognizing non-electrolytes is essential for determining which substances will not produce conductive solutions.
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02:29Weak Bases and Non-Electrolytes
Dissociation in Water
Dissociation in water refers to the process where ionic compounds break apart into their constituent ions when mixed with water. This process is key to understanding how different substances behave in aqueous solutions. For instance, Na2SO4 dissociates into Na+ and SO4^2- ions, contributing to electrical conductivity, while non-ionic compounds like CH3OH do not.
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04:52Percent Dissociation Example
Related Practice
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
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.) What are the molar concentrations of A ions and X ions in a 0.500 M solution of AX3? (LO 4.7)(a) 0.500 M A and 0.500 M X (b) 0.500 M A and 0.167 M X (c) 1.500 M A and 0.500 M X (d) 0.500 M A and 1.500 M X
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Textbook Question
Which of the following solutions will not form a precipitate when added to 10 mL of 0.10 M KOH? (LO 4.10, 4.11)(a) 10 mL of 0.10 NH4Cl (b) 10 mL of 0.10 M PbSO4 (c) 10 mL of 0.10 M Fe(NO3)3 (d) 10 mL of 0.10 M AgCH3CO2
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Textbook Question
Write a net ionic equation for the reaction that occurs when 10 mL of 0.5 M ammonium carbonate is mixed with 10 mL of 0.5 M silver nitrate. (LO 4.9, 4.11) (a) (b) (c) (d) A net ionic reaction cannot be written because a reaction does not take place.
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Textbook Question
When 75.0 mL of a 0.100 M lead(II) nitrate solution is mixed with 100.0 mL of a 0.190 M potassium iodide solu-tion, a yellow-orange precipitate of lead(II) iodide is formed. What is the mass in grams of lead(II) iodide formed? Assume the reaction goes to completion. (LO 4.11, 4.15)(a) 1.729 g(b) 3.458 g(c) 4.380 g (d) 8.760 g
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