A student pours a clear solution of aqueous sodium chloride into a beaker that…
CHEMISTRY · Multi-part · AP · Chemistry · Chemical Reactions · Chemical Reactions
Problem
A student pours a clear solution of aqueous sodium chloride into a beaker that already contains an equal volume of aqueous silver(I) nitrate. Within seconds, a curdy white solid forms and settles to the bottom of the beaker while the supernatant liquid remains colorless.
(a) Write the balanced molecular equation for the reaction that occurs in the beaker, including physical states.
(b) Rewrite the reaction from part (a) as a complete ionic equation. Clearly show all ions that are present in aqueous solution.
(c) Identify the spectator ion(s) in the reaction mixture and explain, in one or two sentences, why each is classified as a spectator based on its behavior at the particulate level.
(d) Write the net ionic equation for the reaction.
(e) Describe a particulate-level sketch (no drawing required) that would represent the contents of the beaker after the reaction is complete. Your description should specify the relative numbers and physical locations (aqueous phase vs. solid phase) of each ionic species present.