For the reaction between 200.0 mL of 0.100 M silver nitrate and 95.00 mL of 0.100 M sodium chloride, the concentration of silver ions in solution after the reaction is complete is
A) 0.00 M. All of the silver ions are used up to make the precipitate.
B) 0.100 M. The silver ions do not participate in the chemical reaction and are considered spectator ions.
C) greater than 0.100 M. For every 1.0 mol of silver nitrate there are 2.0 mol of silver ions in solution.
D) less than 0.100 M. Even though silver ions do not react, they are diluted when mixed with the sodium chloride solution.
E) less than 0.100 M. Some, but not all, of the silver ions are used to make the precipitate.

Question

Quizplus · Accepted Answer

Silver nitrate (AgNO3) reacts with sodium chloride (NaCl) to form silver chloride (AgCl) precipitate and sodium nitrate (NaNO3) in solution. This reaction consumes silver ions to form the precipitate, reducing their concentration in the solution. However, not all silver ions may be used up if one reactant is limiting, leading to a concentration of silver ions that is less than the initial but not zero.

For the Reaction Between 200