Skip to main content
Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 87a
Capitolo 17, Problema 87a

Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. AgBr

Guida verificata passo dopo passo
1
Identify the Ksp value for AgBr from Table 17.2. Ksp (solubility product constant) represents the product of the concentrations of the ions in a saturated solution of a sparingly soluble salt.
Write the dissolution equation for AgBr. AgBr dissolves in water according to the equation: \( AgBr(s) \rightleftharpoons Ag^+(aq) + Br^-(aq) \).
Set up the expression for Ksp based on the dissolution equation. For AgBr, the Ksp expression is \( Ksp = [Ag^+][Br^-] \).
Assume the molar solubility of AgBr is 's'. This means that if 's' moles of AgBr dissolve, it will produce 's' moles of Ag+ and 's' moles of Br- in solution.
Substitute 's' into the Ksp expression and solve for 's'. The equation becomes \( Ksp = s \times s = s^2 \). Solving for 's' will give the molar solubility of AgBr in pure water.

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:
1m

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 quantifies the solubility of a sparingly soluble ionic compound. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. For example, for AgBr, Ksp = [Ag+][Br-]. Understanding Ksp is essential for calculating the molar solubility of compounds in water.
Video consigliato:
Percorso guidato
01:47
Solubility Product Constant

Molar Solubility

Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at equilibrium, expressed in moles per liter (M). It is directly related to Ksp, as the molar solubility can be derived from the Ksp expression by substituting the concentrations of the ions in terms of the solubility. This concept is crucial for determining how much of a compound can dissolve in water.
Video consigliato:
Percorso guidato
04:13
Molar Solubility Example

Dissolution Equilibrium

Dissolution equilibrium describes the dynamic balance between the solid phase of a solute and its ions in solution. When a solid ionic compound like AgBr dissolves, it dissociates into its constituent ions, and the process reaches equilibrium when the rate of dissolution equals the rate of precipitation. Understanding this equilibrium is vital for calculating molar solubility and interpreting Ksp values.
Video consigliato:
Percorso guidato
02:35
Thermal Equilibrium
Pratica correlata
Domanda del libro di testo

Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. b. Mg(OH)2 c. CaF2

Domanda del libro di testo

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. b. PbBr2

339
views
Domanda del libro di testo

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M

479
views
Domanda del libro di testo

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag2CrO4

712
views
1
rank
Domanda del libro di testo

Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. CaCO3 b. PbCl2 c. AgI

Domanda del libro di testo

Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. MX (Ksp = 1.27⨉10-36) b. Ag2CrO4 c. Ca(OH)2