# Determine the concentration of strontium ions in saturated solution of strontium sulfate, SrSO4, if the Ksp for SrSO4 is 3.2×10-7.​

Question

Determine the concentration of strontium ions in saturated solution of strontium sulfate, SrSO4, if the Ksp for SrSO4 is 3.2×10-7.​

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1 year 2021-09-02T21:20:13+00:00 1 Answers 4 views 0

$$[Sr^{2+}]=5.66×10^{-4}M$$

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:

$$Ksp=s*s=s^2\\\\3.2×10^{-7}=s^2$$

Then, we apply the square root to obtain:

$$s=\sqrt{3.2×10^{-7}}\\\\s=5.66×10^{-4}M$$

Which is also the concentration of strontium ions:

$$[Sr^{2+}]=5.66×10^{-4}M$$

Best regards!