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-
To calculate the concentration of NO3- ions in solution C, we need to first determine how many moles of NO3- ions are present in each solution.
In solution A:
We have 3.00 L of a 3.00 M solution of NaCl(aq), which means there are 3.00 moles of NaCl in this solution. Since NaCl dissociates into one Na+ ion and one Cl- ion, there are also 3.00 moles of Cl- ions in this solution.
In solution B:
We have 2.00 L of a 2.00 M solution of AgNO3(aq), which means there are 4.00 moles of AgNO3 in this solution. Since AgNO3 dissociates into one Ag+ ion and one NO3- ion, there are also 4.00 moles of NO3- ions in this solution.
When these solutions are mixed together to form solution C, the Cl- ions from solution A will react with the Ag+ ions from solution B to form a precipitate of AgCl. Since AgCl is insoluble in water, it will separate from the solution. Therefore, the concentration of Cl- ions in solution C will be zero.
On the other hand, the NO3- ions will remain in solution C, as they do not react to form a precipitate. The concentration of NO3- ions in solution C will be the same as the concentration in solution B, which is 2.00 M.
Therefore, the concentration of NO3- ions in solution C is 2.00 M.