Question

What is the Molarity of a 6.3 L dilution of a 0.99Molar solution 3.4 L

Answer 1

0.534 M.

Step-by-step explanation:

Molarity is a measure of the concentration of a solution, defined as the number of moles of solute per liter of solution. When a solution is diluted by adding more solvent, the number of moles of solute remains the same, but the volume of the solution increases, resulting in lower molarity.

In this case, you have a 3.4 L solution with a molarity of 0.99 M. This means that the number of moles of solute in this solution is 3.4 L * 0.99 mol/L = 3.366 moles.

If you dilute this solution to a final volume of 6.3 L by adding more solvent, the number of moles of solute remains the same (3.366 moles), but the volume has increased to 6.3 L. So the molarity of the diluted solution is 3.366 moles / 6.3 L = 0.534 M.

Answer 2

To solve this problem, we can use the dilution formula: M1V1 = M2V2 Where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume. We are given that the initial molarity is 0.99M and the initial volume is 3.4 L. We can use this information to find M2: M1V1 = M2V2 (0.99M)(3.4 L) = M2(6.3 L) M2 = (0.99M)(3.4 L) / (6.3 L) M2 = 0.5357 M Therefore, the molarity of a 6.3 L dilution of a 0.99M solution with an initial volume of