Ch.4 - Reactions in Aqueous Solution

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 33a

Chapter 4, Problem 33a

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

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Sulfuric acid (H_2SO_4) is a strong acid commonly used in various chemical processes.

The term 'monoprotic' refers to an acid that can donate only one proton (H^+) per molecule in an aqueous solution.

To determine if sulfuric acid is monoprotic, consider its chemical formula, H_2SO_4, which indicates it has two hydrogen atoms that can potentially be donated as protons.

In aqueous solution, sulfuric acid dissociates in two steps: the first step involves the donation of one proton, forming the bisulfate ion (HSO_4^-), and the second step involves the donation of a second proton, forming the sulfate ion (SO_4^{2-}).

Since sulfuric acid can donate two protons, it is classified as a diprotic acid, not a monoprotic acid. Therefore, the statement is false.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Monoprotic Acids

Monoprotic acids are acids that can donate only one proton (H⁺ ion) per molecule during the process of dissociation in an aqueous solution. This characteristic is crucial for understanding the acid's strength and behavior in chemical reactions. Examples of monoprotic acids include hydrochloric acid (HCl) and acetic acid (CH₃COOH).

Sulfuric Acid

Sulfuric acid (H₂SO₄) is a strong diprotic acid, meaning it can donate two protons per molecule. The first dissociation releases one proton, while the second dissociation releases another proton, making it capable of acting as both a monoprotic and diprotic acid depending on the context. This property is essential for understanding its reactivity and applications in various chemical processes.

Acid Strength and Classification

Acid strength refers to the ability of an acid to donate protons in solution, which is influenced by its molecular structure and the stability of its conjugate base. Acids are classified as strong or weak based on their degree of ionization in water. Understanding this classification helps in predicting the behavior of acids in chemical reactions and their interactions with bases.

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Textbook Question

Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?

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Textbook Question

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

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Textbook Question

Which of the following solutions is the most basic? a. 0.6𝑀 NH3 b. 0.150 M KOH c. 0.100𝑀Ba(OH)2

Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case.

(c) Although sulfuric acid is a strong electrolyte, an aqueous solution of H₂SO₄ contains more HSO₄^- ions than SO₄^2- ions.

You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3,CaCl2, or Al2(SO4)3. You take a portion of the solution and add an aqueous solution of Ba(NO3)2 to it, and observe that a white solid precipitates Then you take another portion of the unlabeled solution and add an aqueous solution of NaCl to it; nothing appears to happen. What is the most likely identity of the solution in the unlabeled bottle: silver nitrate, calcium chloride, aluminum sulfate?

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Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case. (c) Methanol is a base.

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