Question

252 mL of 3,00 M H2SO4 are added to 1,50 L of 0,500 M H2SO4. What is the concentration of the resulting solution?)

Answer 1

If 252 mL of 3.00 M H₂SO₄ are added to 1.50 L of 0.500 M H₂SO₄. The concentration of the resulting solution can be calculated as follows:

Molarity = moles / liter

The first step is to find the number of moles of the individual solutions.

The number of liters contained in Solutions 1 and 2 is calculated. Convert the volume of solution in mL to the units of liters (L). Then we can calculate the number of moles of H₂SO₄ contained in solutions 1 and 2.

Moles can be calculated using the following formula: moles = molarity * volume

Number of moles of H₂SO₄ in solution 1 = 3.00 M 0.252 L = 0.756 moles

For Solution 2, moles of H₂SO₄ = 0.5 M 1.5 L = 0.75 moles

Summing up the two values to get the total number of moles. In this case, 0.756+0.75 = 1.506 moles of H₂SO₄

Summing up the volumes of solutions to determine the final volume. So, for solution 1 is 0.252 L and solution 2 is 1.5 L. Hence the final volume = 0.252 L + 1.5 L = 1.752 L.

Therefore, we can calculate the final molarity of the mixed solution using the equation molarity = moles / liter.

Hence the the final molarity is 1.506 moles 1.752 L = 0.86 M