Two solutions of a substance (non-electrolyte) are mixed in the following manner. 480 mL of 1.5 M first solution +520 mL of 1.2 M second solution. What is the molarity of the final mixture?

1.344 M

The correct answer is option 1. 1.344 M.

To find the molarity of the final mixture after mixing two solutions, we need to use the formula that relates the molarity of solutions to their volumes and concentrations.

Let us calculate step by step:

For the first solution:

\(\text{Moles of solute from first solution} = \text{Molarity} \times \text{Volume in liters}\)

\(\text{Moles of solute from first solution} = 1.5 \, \text{M} \times 0.480 \, \text{L} = 0.72 \, \text{moles}\)

For the second solution:

\(\text{Moles of solute from second solution} = \text{Molarity} \times \text{Volume in liters}\)

\(\text{Moles of solute from second solution} = 1.2 \, \text{M} \times 0.520 \, \text{L} = 0.624 \, \text{moles}\)

\(\text{Total moles of solute} = 0.72 \, \text{moles} + 0.624 \, \text{moles} = 1.344 \, \text{moles}\)

\(\text{Total volume of the mixture} = 480 \, \text{mL} + 520 \, \text{mL} = 1000 \, \text{mL} = 1.000 \, \text{L}\)

\(\text{Molarity} = \frac{\text{Total moles of solute}}{\text{Total volume of mixture in liters}}\)

\(\text{Molarity} = \frac{1.344 \, \text{moles}}{1.000 \, \text{L}} = 1.344 \, \text{M}\)

Conclusion:

Therefore, the molarity of the final mixture is 1.344 M.