Skip to main content
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 74c
Capitolo 17, Problema 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?

Guida verificata passo dopo passo
1
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.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
6m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

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.
Video consigliato:
Percorso guidato
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.
Video consigliato:
Percorso guidato
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.
Video consigliato:
Percorso guidato
01:16
Stoichiometry Concept
Pratica correlata
Domanda del libro di testo

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.)

1427
views
Domanda del libro di testo

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+?

696
views
1
rank
Domanda del libro di testo

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?

617
views