Respuesta :
Answer:
The equilibrium constant Ksp of the generic salt AB2 = 6.4777 *10^-8 M
Explanation:
Step 1: The balanced equation
AB2 ⇒ A2+ + 2B-
Step 2: Given data
Concentration of A2+ = 0.00253 M
Concentration of B- = 0.00506 M
Step 3: Calculate the equilibrium constant
Equilibrium constant Ksp of [AB2] = [A2+][B-]²
Ksp = 0.00253 * 0.00506² = 6.4777 *10^-8 M
The equilibrium constant Ksp of the generic salt AB2 = 6.4777 *10^-8 M
Answer:
[tex]6.477\times 10^{-7}[/tex] is the equilibrium constant, [tex]K_{sp}[/tex], of the generic salt [tex]AB_2[/tex].
Explanation:
Solubility product constant : It is defined as the product of the concentration of the ions present in a solution raised to the power by its stoichiometric coefficient in a solution of a salt. This takes place at equilibrium only. The solubility product constant is represented as, [tex]K__{sp}[/tex].
[tex]A_xB_y\rightleftharpoons xA^{y+}+yB^{x-}[/tex]
[tex]K_{sp}=[A^{y+}]^x\times [B^{x-}]^y[/tex]
Equilibrium concentration for a generic cation = [tex][A^{2+}]=0.00253 M[/tex]
Equilibrium concentration for a generic anion = [tex][B^{-}]=0.00506 M[/tex]
[tex]AB^2\rightleftharpoons A^{2+}+2B^-[/tex]
The expression of solubility product is given as:
[tex]K_{sp}=[A^{2+}][[B^-]]^2[/tex]
[tex]K_{sp}=0.00253 M\times (0.00506 M)^2=6.477\times 10^{-7}[/tex]
[tex]6.477\times 10^{-7}[/tex] is the equilibrium constant, [tex]K_{sp}[/tex], of the generic salt [tex]AB_2[/tex].
