Question

Determine the concentration of strontium ions in saturated solution of strontium sulfate, SrSO4, if the Ksp for SrSO4 is 3.2x10-7.​

Answer 1

`[Sr^(2+)]=5.66x10^(-4)M`

Step-by-step explanation:

Hello there!

In this case, given the solubility equilibrium of strontium sulfate:

`SrSO_4(s)\rightleftharpoons Sr^(2+)(aq)+SO_4^(2-)(aq)`

Whose equilibrium expression is:

`Ksp=[Sr^(2+)][SO_4^(2-)]`

In such a way, we can introduce the molar solubility, s, in the equation to obtain:

`Ksp=s*s=s^2\\\\3.2x10^(-7)=s^2`

Then, we apply the square root to obtain:

`s=\sqrt{3.2x10^(-7)}\\\\s=5.66x10^(-4)M`

Which is also the concentration of strontium ions:

`[Sr^(2+)]=5.66x10^(-4)M`

Best regards!