Final answer:
The molarity of the diluted solution after adding 27.5 mL of 16.0 M nitric acid stock solution to 300 mL of water is 1.34 M.
Step-by-step explanation:
The student is asking about how the molarity of a nitric acid solution changes after dilution. To find the molarity of the diluted solution, we use the formula M1V1 = M2V2, where M1 and V1 represent the molarity and volume of the concentrated solution, and M2 and V2 represent the molarity and volume of the diluted solution.
In this case, the initial concentration (M1) is 16.0 M and the initial volume (V1) is 27.5 mL. The final volume (V2) after dilution is the sum of the volume of the stock solution plus the volume of water added, which is 27.5 mL + 300 mL = 327.5 mL. We are solving for the final concentration (M2).
Applying the dilution formula: (16.0 M) × (27.5 mL) = M2 × (327.5 mL). Dividing both sides of the equation by 327.5 mL, we get M2 = (16.0 M × 27.5 mL) / 327.5 mL.
Performing the calculation:
M2 = (16.0 × 27.5) / 327.5
M2 = 1.34 M, which is the molarity of the diluted solution.