Question

At 25 °C, an aqueous solution has an equilibrium concentration of 0.00253 M for a generic cation, A2+(aq), and 0.00506 M for a generic anion, B−(aq). What is the equilibrium constant, Ksp, of the generic salt AB2(s)? Ksp=At 25 °C, an aqueous solution has an equilibrium concentration of 0.00253 M for a generic cation, A2+(aq), and 0.00506 M for a generic anion, B−(aq). What is the equilibrium constant, Ksp, of the generic salt AB2(s)? Ksp=

Answer 1

`6.477* 10^(-7)` is the equilibrium constant,
`K_(sp)`, of the generic salt
`AB_2`.

Step-by-step 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,
`K__(sp)`.

`A_xB_y\rightleftharpoons xA^(y+)+yB^(x-)`

`K_(sp)=[A^(y+)]^x* [B^(x-)]^y`

Equilibrium concentration for a generic cation =
`[A^(2+)]=0.00253 M`

Equilibrium concentration for a generic anion =
`[B^(-)]=0.00506 M`

`AB^2\rightleftharpoons A^(2+)+2B^-`

The expression of solubility product is given as:

`K_(sp)=[A^(2+)][[B^-]]^2`

`K_(sp)=0.00253 M* (0.00506 M)^2=6.477* 10^(-7)`

`6.477* 10^(-7)` is the equilibrium constant,
`K_(sp)`, of the generic salt
`AB_2`.

Answer 2

The equilibrium constant Ksp of the generic salt AB2 = 6.4777 *10^-8 M

Step-by-step 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