You have 3.00 L of a 3.00 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO3(aq) called solution B. You mix these solutions together, making solution C. Hint: AgCl is a precipitate.
Calculate the concentrations (in M) of the following ions in solution C.
NO3-
Group of answer choices
1.00 M
1.80 M
0 M
1.50 M
0.800 M
To calculate the concentration of ions in solution C, we need to consider the reaction that occurs when NaCl(aq) and AgNO3(aq) are mixed together:
NaCl(aq) + AgNO3(aq) -> AgCl(s) + NaNO3(aq)
From the balanced equation, we can see that AgCl is formed as a precipitate, while NaNO3 remains in the solution.
Since AgCl is insoluble and forms a solid precipitate, it does not dissociate into ions. Therefore, the concentration of Ag+ ions in solution C is 0 M.
On the other hand, NaNO3 dissociates completely in solution, resulting in the same concentration of NO3- ions as the original NaNO3 solution. The concentration of NO3- ions in solution C is therefore 2.00 M.
In conclusion, the concentration of NO3- ions in solution C is 2.00 M, while the concentration of Ag+ ions is 0 M. Therefore, the correct answer is 0 M.