Problem: A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+.How much Na2SO4 solution must be added to initiate the precipitation?

🤓 Based on our data, we think this question is relevant for Professor Jana & Bouchard's class at MASS PHARM.

FREE Expert Solution

Recall:

Ksp=productsreactants

Ksp[Ca2+]=[Ca2+][SO42-][Ca2+][SO42-]=Ksp[Ca2+]

[SO42-]=7.1×10-50.20 M=3.55×10-4 M

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Problem Details

A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+.

How much Na2SO4 solution must be added to initiate the precipitation?

Frequently Asked Questions

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 Selective Precipitation concept. If you need more Selective Precipitation practice, you can also practice Selective Precipitation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Jana & Bouchard's class at MASS PHARM.