molarity of no-3 in solution after 2 liters of 3 m agno3 mixed with 3 liters 1 mbacl2

To find the molarity of nitrate ions (NO3-) in the solution after mixing 2 liters of 3 M AgNO3 with 3 liters of 1 M BaCl2, we first need to determine how many moles of nitrate ions are present in the AgNO3 solution and then calculate the total volume of the mixed solution.

Step 1: Calculate Moles of Nitrate from AgNO3

AgNO3 dissociates in solution to produce one mole of nitrate ions for each mole of AgNO3. Therefore, we can calculate the moles of AgNO3 in the 2 liters of 3 M solution as follows:

• Moles of AgNO3: Molarity (M) × Volume (L) = 3 moles/L × 2 L = 6 moles
• Moles of NO3-: Since each mole of AgNO3 gives one mole of NO3-, we also have 6 moles of NO3-.

Step 2: Calculate Total Volume of the Mixed Solution

Next, we need to find the total volume of the solution after mixing the two solutions:

• Volume of AgNO3 solution: 2 L
• Volume of BaCl2 solution: 3 L
• Total Volume: 2 L + 3 L = 5 L

Step 3: Calculate Molarity of Nitrate Ions

Now that we know the total moles of nitrate ions and the total volume of the solution, we can calculate the molarity of the nitrate ions:

• Molarity of NO3-: Moles of NO3- / Total Volume = 6 moles / 5 L = 1.2 M

Final Result

Therefore, the molarity of nitrate ions (NO3-) in the final solution after mixing is 1.2 M. This calculation shows how to combine solutions and determine the concentration of specific ions in a mixture, which is a fundamental concept in chemistry.