Answer :

Final answer:

The molarity of a solution obtained by mixing 100 ml of 0.3M H₂SO₄ and 200 ml of 1.5M H₂SO₄ is calculated by first finding the total moles of H₂SO₄ in each solution and summing them. The total molarity is then found by dividing the total moles by the total volume in liters, giving a final molarity of 1.1M.

Explanation:

To calculate the molarity of a mixed solution, we first need to calculate the total moles of the solute (H₂SO₄). We do this by multiplying the molarity of each individual solution by its volume. Thus, moles of H₂SO₄ in 0.3M solution = 0.3 moles/liter * 0.1 liters = 0.03 moles. Similarly, for the 1.5M solution we have 1.5 moles/liter * 0.2 liters = 0.3 moles.

The total moles in the solution is then the sum of the moles in each solution: 0.03 moles + 0.3 moles = 0.33 moles.

The molarity of the mixed solution is calculated by dividing the total moles by the total volume of the solution (in liters). In this case, the total volume is 100 ml + 200 ml = 300 ml = 0.3 liters. Thus, the molarity is 0.33 moles / 0.3 liters = 1.1M.

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