1. Does bubbling ammonia through a solution raise or lower the pH? Explain 2. A
ID: 1081830 • Letter: 1
Question
1. Does bubbling ammonia through a solution raise or lower the pH? Explain 2. A chemist knows that a solution contains metal ions. She adds sodium chloride to the solution for solubility and observes a precipitate. List all of the possible precipitates. Consult your text rules if necessary 3. A chemist adds lithium carbonate to a solution of calcium chloride. A precipitate forms. The chemist then adds nitric acid to the solution. Bubbles evolve, and the precipitate disappears. Give the net ionic equation for the precipitation reaction and the net ionic equation of the reaction that leads to the disappearance of the precipitate.Explanation / Answer
Ans. #1. Ammonia (NH3) when bubbled through a solution, forms ammonium hydroxide (NH4OH). NH4OH further dissociates to release OH- in the solution as follow-
NH3 + H2O ----> NH4OH <-------> NH4+ + OH-
Formation of OH- in the solution makes the solution alkaline or basic.
Bubbling NH3 through a solution increase its pH (make it basic or alkaline).
#2. NaCl releases chloride ions (Cl-) in the solution.
Solubility rule: The chlorides of Cu, Pb, Hg and Ag are insoluble (Note: PbCl2 is springily soluble).
So, list of possible precipitates are- CuCl2, PbCl2, HgCl, AgCl.
#3. Reaction 1: Balanced reaction:
2 Li2CO3(aq) + CaCl2(aq) ---------> 2 LiCl + CaCO3(s)
Net ionic reaction: CO32-(aq) + Ca2+(aq) ---------> CaCO3(s)
# Reaction 2: Balanced reaction:
CaCO3(s) + 2 HNO3(aq) -------> Ca(NO3)2(aq) + H2O(l) + CO2(g)
Net ionic reaction: Write all the components in the balanced reaction in ionic form, if possible (don’t write the solid forms in ionic form).
CaCO3(s) + 2H+(aq) + 2NO3-(aq) -------> Ca2+(aq) + 2NO3-(aq) + 2H+ + 2OH- + CO2(g)
# Cancel the terms common on either side of the reaction. The remaining reaction is the net ionic reaction.
Net ionic reaction: CaCO3(s) -------> Ca2+(aq) + 2OH- + CO2(g)
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