Problem: A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.Write net ionic equations for the formation of each of the precipitates observed.

🤓 Based on our data, we think this question is relevant for Professor Siler's class at OREGONSTATE.

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Addition of sodium sulfate (Na2SO4)

Sulfides (S2-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+

Na2SO4(aq) + 2 Ag+(aq) →  Ag2SO4(s) + 2 Na+(aq) 

 Ag2SO4(aq) → insoluble

Na2SO4(aq) + Ca2+(aq) → CaSO4(s) + 2 Na+(aq) 

CaSO4(s) → soluble

Na2SO4(aq) + Cu2+ → CuSO4(s) + 2 Na+(aq) 

CuSO4(s) → insoluble


Addition of sodium carbonate (Na2CO3):

Carbonates (CO32-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+)

Na2CO3(aq) + Ca2+(aq) → CaCO3(s) + 2 Na+(aq) 

CaCO3(s) → insoluble


Net ionic equations:

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Problem Details

A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.

Write net ionic equations for the formation of each of the precipitates observed.

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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 Net Ionic Equations concept. You can view video lessons to learn Net Ionic Equations. Or if you need more Net Ionic Equations practice, you can also practice Net Ionic Equations practice problems.

What professor is this problem relevant for?

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