Question

a dilute solution is prepared by transferring 40.00 mL of a 0.4433 M stock solution to a 750.0 mL volumetric flask and diluting to mark. what is the molarity of this dilute solution?

Answer 1

Answer: 0.0236 M

Step-by-step explanation:

To find the molarity of the dilute solution, we can use the formula:

Molarity (M) = (Moles of solute) / (Volume of solution in liters)

First, let's calculate the moles of solute (stock solution) using the given information:

1. Convert the volume of the stock solution to liters:

40.00 mL = 40.00 mL / 1000 mL/L = 0.0400 L

2. Use the molarity of the stock solution to calculate the moles of solute:

Moles of solute = Molarity × Volume of solution

Moles of solute = 0.4433 M × 0.0400 L = 0.0177 moles

Now, let's find the volume of the dilute solution:

The dilute solution is prepared in a 750.0 mL volumetric flask and diluted to the mark. This means that the final volume of the solution is 750.0 mL.

3. Convert the volume of the dilute solution to liters:

750.0 mL = 750.0 mL / 1000 mL/L = 0.750 L

Finally, we can use the formula to calculate the molarity of the dilute solution:

Molarity (dilute solution) = (Moles of solute) / (Volume of solution)

Molarity (dilute solution) = 0.0177 moles / 0.750 L = 0.0236 M

Therefore, the molarity of the dilute solution is 0.0236 M.

I hope this helps :)