# Problem: The Ksp of CaSO4 is 4.93 x 10-5. Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO4 (aq) at 25 °C.

###### FREE Expert Solution
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###### FREE Expert Solution

For this problem, we’re being asked to calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO4(aq). Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of CaSO4 and Na2SO4 in water are as follows:

The sulfate ion, SO42–, has a charge of –2. Calcium is in Group 2A so it’s charge is +2:

CaSO4(s)  Ca2+(aq) + SO42–(aq)

The sulfate ion, SO42–, has a charge of –2. Sodium is in Group 1A so it’s charge is +1:

Na2SO4(s)  2 Na+(aq) + SO42–(aq)

Notice that there is a common ion present, SO42–. The common ion effect states that the solubility of a salt is lower in the presence of a common ion.

We can construct an ICE table for the dissociation of CaSO4. Remember that solids are ignored in the ICE table.

99% (393 ratings)
###### Problem Details

The Ksp of CaSO4 is 4.93 x 10-5. Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO(aq) at 25 °C.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.

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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.