Question

Solid strontium chromate, SrCrO4, dissolves into its respective ions at 25°C. Suppose that in a particular solution, [Sr^2+]=6.0x10^-3M. Find the value of Ksp.

A) 3.6 x 10^-5
B) 6.0 x 10^-3
C) 3.6 x 10^-2
D) 7.7 x 10^-2

Answer 1

A) 3.6 x 10^-5.

Step-by-step explanation:

Hello there!

In this case, according to the given information, it turns out firstly necessary to write the equilibrium expression for the dissociation of strontium chromate:

`Ksp=[Sr^(2+)][CrO_4^(2-)]`

Thus, since strontium and chromate ions are in a 1:1 mole ratio, we can tell the concentration of both ions as the same; and therefore, the Ksp is:

`Ksp=(6.0x10^(-3)M)(6.0x10^(-3)M)\\\\Ksp=3.6x10^(-5)`

Or option A) 3.6 x 10^-5.

Regards!