Question

A salt has the formula AB2, and a Ksp value of 4.3 × 10-7. What is the solubility of the salt? A. 6.5 × 10-3 Molar B. 4.8 × 10-4 Molar C. 4.8 × 10-3 Molar D. 7.5 × 10-3 Molar

Answer 1

C. 4.8 x 10 -3

Step-by-step explanation:

plato

Answer 2

Answer: The solubility of the salt is
`4.8* 10^(-3)M`

Step-by-step explanation:

Solubility product is defined as the equilibrium constant in which a solid ionic compound is dissolved to produce its ions in solution. It is represented as
`K_(sp)`

The equation for the reaction will be as follows:

`AB_2\rightleftharpoons A^(2+)+2B^-`

By Stoichiometry,

1 mole of
`AB_2` gives 1 mole of
`A^(2+)` and 2 moles of
`B^-`

Thus if solubility of
`AB_2` is s moles/liter, solubility of
`A^(2+)` is s moles\liter and solubility of
`B^-` is 2s moles/liter

Therefore,

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

`4.3* 10^(-7)=[s][2s]^2`

`4s^3=4.3* 10^(-7)`

`s=4.8* 10^(-3)M`

The solubility of the salt is
`4.8* 10^(-3)M`