Skip to main content
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 62b
Capitolo 17, Problema 62b

Calculate the molar solubility of Ni(OH)2 when buffered at pH (b) 10.0.

Guida verificata passo dopo passo
1
Identify the dissolution equation for Ni(OH)_2: Ni(OH)_2(s) \(\rightleftharpoons\) Ni^{2+}(aq) + 2OH^{-}(aq).
Write the expression for the solubility product constant (K_{sp}) for Ni(OH)_2: K_{sp} = [Ni^{2+}][OH^{-}]^2.
Determine the concentration of OH^{-} ions from the given pH: Use the relation pOH = 14 - pH to find pOH, then calculate [OH^{-}] = 10^{-pOH}.
Substitute the [OH^{-}] value into the K_{sp} expression and solve for [Ni^{2+}], which represents the molar solubility of Ni(OH)_2.
Use the known K_{sp} value for Ni(OH)_2 to calculate the molar solubility by substituting the [OH^{-}] concentration and solving for [Ni^{2+}].

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:
7m

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 given volume of solvent at a specific temperature, expressed in moles per liter (mol/L). It is a crucial concept in understanding how substances interact in solution, particularly for sparingly soluble compounds like Ni(OH)2. The molar solubility can be influenced by factors such as pH, temperature, and the presence of other ions in solution.
Video consigliato:
Percorso guidato
04:13
Molar Solubility Example

pH and its Effect on Solubility

pH is a measure of the acidity or basicity of a solution, which can significantly affect the solubility of certain compounds. For nickel(II) hydroxide, Ni(OH)2, an increase in pH (making the solution more basic) can enhance its solubility due to the formation of soluble nickel complexes. Understanding how pH influences the dissociation of hydroxides is essential for calculating molar solubility in buffered solutions.
Video consigliato:
Percorso guidato
05:30
Solubility at Buffered pH Example

Equilibrium and Ksp

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. For Ni(OH)2, the Ksp expression relates the concentrations of the ions in solution at equilibrium. By knowing the Ksp value and the pH of the solution, one can derive the molar solubility by setting up an equilibrium expression that accounts for the concentration of hydroxide ions, which are influenced by the pH.
Video consigliato:
Percorso guidato
01:51
Ksp Calculations
Pratica correlata
Domanda del libro di testo

Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF21s2. Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF2 at the bottom of the beaker increase, decrease, or remain the same?

1186
views
Domanda del libro di testo

Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0 (b) 9.5 (c) 11.8.

600
views
Domanda del libro di testo

For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS (b) PbF2 (c) AuCl3 (e) CuBr (d) Hg2C2O4.

917
views
Domanda del libro di testo

Calculate the molar solubility of Ni(OH)2 when buffered at pH (c) 12.0.

330
views
Domanda del libro di testo

Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0.

741
views