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 96a
Capitolo 17, Problema 96a

Calculate the molar solubility of MX (Ksp = 1.27 × 10^-36) in pure water.

Guida verificata passo dopo passo
1
Identify the dissociation equation for the salt MX: MX(s) \(\rightleftharpoons\) M^+(aq) + X^-(aq).
Write the expression for the solubility product constant (K_{sp}): K_{sp} = [M^+][X^-].
Assume the molar solubility of MX is 's'. Therefore, [M^+] = s and [X^-] = s.
Substitute the concentrations into the K_{sp} expression: K_{sp} = s \(\times\) s = s^2.
Solve for 's' by taking the square root of both sides: s = \(\sqrt{K_{sp}\)}.

Concetti chiave

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

Molar Solubility

Molar solubility refers to the maximum amount of a solute that can dissolve in a solvent at a given temperature, expressed in moles per liter (mol/L). It is a critical concept in understanding how ionic compounds dissociate in solution and is often determined from the solubility product constant (Ksp). For a compound MX, the molar solubility can be calculated by setting up an equilibrium expression based on its dissociation in water.
Video consigliato:
Percorso guidato
04:13
Molar Solubility Example

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 MX, Ksp = [M^+] [X^-], where [M^+] and [X^-] are the molar concentrations of the ions in solution, allowing for the calculation of molar solubility.
Video consigliato:
Percorso guidato
01:47
Solubility Product Constant

Dissociation of Ionic Compounds

Dissociation of ionic compounds occurs when they dissolve in water, breaking apart into their constituent ions. For example, when MX dissolves, it separates into M^+ and X^- ions. This process is essential for calculating molar solubility, as the concentration of each ion at equilibrium directly influences the Ksp value. Understanding this dissociation helps in setting up the equilibrium expression needed to find the molar solubility from the given Ksp.
Video consigliato:
Percorso guidato
02:11
Ionic Compounds Naming
Pratica correlata
Domanda del libro di testo

Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2

738
views
Domanda del libro di testo

Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water

796
views
Domanda del libro di testo

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4

2628
views
Domanda del libro di testo

Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF

639
views
Domanda del libro di testo

Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2

2358
views
1
comments
Domanda del libro di testo

Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. c. 0.20 M Na2X

2231
views