We are asked to identify the precipitate formed when two salts are mixed together. We will refer to the solubility rules in order to determine if an insoluble product (precipitate) is formed or not.
•Soluble Ionic Compounds:
▪ Group 1A ions (Li+, Na+, K+, etc.) and Ammonium ion (NH4+) are soluble
▪ Nitrates (NO3-), Acetates (CH3COO- or C2H3O2-), and most Perchlorates (ClO4-) are soluble
▪ Cl-, Br-, and I- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+
▪ Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+
• Insoluble Ionic Compounds:
Which of these processes will occur if solutions of Li2CO3(aq) and CdCl2(aq) are mixed?
A. LiCl will precipitate; Cd2+ and CO32- are spectator ions.
B. CdCl2 will precipitate; Li+ and CO32- are spectator ions.
C. Li2CO3 will precipitate; Cd2+ and Cl- are spectator ions.
D. CdCO3 will precipitate; Li+ and Cl- are spectator ions.
E. No precipitate will form.
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 Solubility Rules concept. You can view video lessons to learn Solubility Rules. Or if you need more Solubility Rules practice, you can also practice Solubility Rules practice problems.