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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.17 - Additional Aspects of Aqueous Equilibria문제 74c
17장, 문제 74c

A solution of Na2SO4 is added dropwise to a solution that is 0.010 M in Ba2+(aq) and 0.010 M in Sr2+(aq). (c) What is the concentration of SO42-(aq) when the second cation begins to precipitate?

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Identify the solubility product constants (Ksp) for the possible precipitates, BaSO4 and SrSO4. These constants help determine the solubility of each salt in water.
Write the solubility product expressions for BaSO4 and SrSO4. For BaSO4, the expression is Ksp = [Ba2+][SO42-], and for SrSO4, it is Ksp = [Sr2+][SO42-].
Calculate the concentration of SO42- required to start precipitation of BaSO4 using the initial concentration of Ba2+ and the Ksp value for BaSO4. This is done by rearranging the solubility product expression to solve for [SO42-].
Similarly, calculate the concentration of SO42- required to start precipitation of SrSO4 using the initial concentration of Sr2+ and the Ksp value for SrSO4.
Compare the calculated concentrations of SO42- for both salts. The second cation begins to precipitate at the higher of the two calculated concentrations, as it indicates the point where the solution becomes saturated with respect to that cation.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of ionic compounds. It represents the maximum concentration of ions in a saturated solution at a given temperature. For a salt like BaSO4 or SrSO4, Ksp values can be used to determine when the solution becomes saturated and precipitation begins, which is crucial for understanding when the second cation will precipitate.
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가이드 코스
01:47
Solubility Product Constant

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble compound, or precipitate. In this case, the addition of Na2SO4 introduces sulfate ions (SO4^2-) that can react with Ba^2+ and Sr^2+ ions to form BaSO4 and SrSO4, respectively. Understanding the conditions under which these precipitates form is essential for determining the concentration of sulfate ions when the second cation begins to precipitate.
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가이드 코스
01:53
Selective Precipitation

Ion Concentration and Stoichiometry

Ion concentration refers to the amount of a specific ion present in a solution, typically expressed in molarity (M). Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In this scenario, knowing the initial concentrations of Ba^2+ and Sr^2+ allows for the calculation of the sulfate ion concentration needed to initiate the precipitation of the second cation, based on the stoichiometric ratios of the reactions.
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가이드 코스
01:16
Stoichiometry Concept
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교과서 질문

A solution of Na2SO4 is added dropwise to a solution that is 0.010 M in Ba2+(aq) and 0.010 M in Sr2+(aq). (a) What concentration of SO42- is necessary to begin precipitation? (Neglect volume changes. BaSO4: Ksp = 1.1⨉10-10; SrSO4: Ksp = 3.2⨉10-7.)

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교과서 질문

A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with (NH4)2HPO4. No precipitate forms. Which of these metal cations are either possibly present or definitely absent: Al3+, Na+, Ag+, Mg2+?

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교과서 질문

A solution of Na2SO4 is added dropwise to a solution that is 0.010 M in Ba2+(aq) and 0.010 M in Sr2+(aq). (b) Which cation precipitates first?

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