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 10b

Chapter 4, Problem 10b

An aqueous solution contains 1.2 mM of total ions. (b) If the solution is FeCl3(aq), what is the concentration of chloride ion?

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Identify the dissociation equation for FeCl_3 in water: FeCl_3(aq) \(\rightarrow\) Fe^{3+}(aq) + 3Cl^{-}(aq).

Recognize that for every 1 mole of FeCl_3 that dissociates, 3 moles of Cl^- ions are produced.

Given that the total concentration of ions is 1.2 mM, determine the concentration of FeCl_3 by considering the stoichiometry of the dissociation.

Calculate the concentration of Cl^- ions by multiplying the concentration of FeCl_3 by 3, as each FeCl_3 produces 3 Cl^- ions.

Express the concentration of Cl^- ions in mM, ensuring the units are consistent with the given total ion concentration.

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Key Concepts

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

Dissociation of Ionic Compounds

Ionic compounds, such as FeCl3, dissociate into their constituent ions when dissolved in water. For FeCl3, it separates into one Fe³⁺ ion and three Cl⁻ ions. Understanding this dissociation is crucial for calculating the concentration of individual ions in a solution.

Molarity and Concentration

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. In this case, the total ion concentration is given in millimoles per liter (mM), which can be converted to moles per liter. This concept is essential for determining the concentration of specific ions in the solution.

Stoichiometry in Solutions

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In the context of this question, it helps to determine the ratio of ions produced from the dissociation of FeCl3, allowing us to calculate the concentration of chloride ions based on the total ion concentration.

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Solution Stoichiometry

Related Practice

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

An aqueous solution contains 1.2 mM of total ions. (a) If the solution is NaCl(aq), what is the concentration of chloride ion?

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Textbook Question

In a titration experiment, 50.0 mL of 0.075 M acetic acid, CH₃COOH, is titrated with the 0.250 M KOH(aq) that is in the burette. The drawing shows the level of the KOH in the burette before the titration begins. What will be the burette reading at the equivalence point?

Textbook Question

What kind of reaction is this? N2(g)+3H2(g)⟶2NH3(g)

a. an acid–base reaction

b. a metathesis reaction

c. a redox reaction

d. a precipitation reaction

Textbook Question

Which of these statements is true?

a. If a compound is oxidized, it is gaining electrons.

b. If a base is neutralized, it is gaining protons.

c. Elements that are metals cannot be oxidized.

d. If hydrogen gas is generated in a reaction, it must be an acid–base reaction.

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.