100 ml each of 1M AgNO₃ and 1M NaCl are mixed. The nitrate ion concentration in the resulting solution is

When two solutions of 1M AgNO₃ and 1M NaCl are mixed in equal volumes, a precipitation reaction occurs. This reaction leads to the formation of a solid precipitate, AgCl (Silver Chloride), while NaNO₃ (Sodium Nitrate) remains dissolved in the solution. The reaction can be represented by the following balanced chemical equation:

AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)

Step-by-Step Calculation

Step 1: Write the balanced chemical equation

The balanced chemical equation for the reaction is:

AgNO₃ (aq) + NaCl (aq) → AgCl (s) + NaNO₃ (aq)

Step 2: Determine the initial moles of AgNO₃

The molarity of AgNO₃ is given as 1M (1 mole per liter). Since we are using 100 mL (0.1 L) of AgNO₃ solution, we can calculate the moles of AgNO₃ in this volume:

Moles of AgNO₃ = Molarity × Volume = 1 M × 0.1 L = 0.1 moles

Step 3: Total volume of the resulting solution

After mixing 100 mL of AgNO₃ solution and 100 mL of NaCl solution, the total volume of the resulting solution becomes:

Total volume = 100 mL + 100 mL = 200 mL = 0.2 L

Step 4: Calculate the concentration of nitrate ions

The nitrate ions come from the dissociation of AgNO₃ and NaNO₃. Since the nitrate ions come solely from the dissociated AgNO₃ (which is converted into NaNO₃ during the reaction), the moles of nitrate ions in the resulting solution will be equal to the moles of AgNO₃, which is 0.1 moles.

The concentration of nitrate ions (NO₃⁻) in the final solution is calculated by dividing the moles of nitrate ions by the total volume of the solution:

Concentration of NO₃⁻ = Moles of NO₃⁻ / Total volume = 0.1 moles / 0.2 L = 0.5 M

Final Answer

The concentration of nitrate ions (NO₃⁻) in the resulting solution is 0.5 M.