Question

3. The following solutions are mixed together: 75.0 mL of 0.100-M lead (II) nitrate 100.0 mL of…

3. The following solutions are mixed together: 75.0 mL of 0.100-M lead (II) nitrate 100.0 mL of 0.190-M potassium iodide
A precipitate of lead (II) iodide is formed in a double displacement reaction. a) Calculate the number of moles of NO3– ions in the resulting solution. (Hint: Thenitrate ions are
spectator ions in this reaction.) b) Write a complete, balanced equation, and then a net ionic equation for this chemical reaction.
Include state symbols such as (s), (aq), etc. c) Calculate the mass of lead (II) iodide which would be formed, assuming the reaction goes to
completion. d) Calculate the molarity of all of the following ions in the resulting solution. (Note: Assuming that
the reaction goes to completion, some of the concentrations may be effectively zero.) i) Pb2+ ii) K+ iii) NO3– iv) I–

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