Question

A chemist adds 0.50L of a 0.485 M copper(II) sulfate CuSO4 solution to a reaction flask. Calculate the millimoles of copper(II) sulfate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Answer 1

The chemist has added 242.5 millimoles of copper(II) sulfate to the flask by converting the volume to milliliters and multiplying by the molarity of the solution.

Step-by-step explanation:

To calculate the number of millimoles of copper(II) sulfate (CuSO4) added by the chemist, we use the concentration of the solution and the volume added. The concentration is given as 0.485 M, which means there are 0.485 moles of CuSO4 per liter of solution. Since 1 mole equals 1000 millimoles, we can first convert the volume from liters to milliliters (0.50 L = 500 mL) and then multiply by the concentration in moles per liter.

The calculation is:
500 mL × 0.485 moles/L = 242.5 millimoles

Therefore, the chemist has added 242.5 millimoles of CuSO4 to the reaction flask.

Answer 2

Step-by-step explanation:

It is given that volume is 0.50 L and molarity is 0.485 M. Hence, number of millimoles will be calculated as follows.

Number of millimoles = Molarity × Volume

As there are 1000 mL in 1 L. So, 0.50 L equals 500 mL.

Therefore, putting the given values into the above formula as follows.

Number of millimoles = Molarity × Volume

= 0.485 M × 500 mL

= 242.5

Thus, we can conclude that 242.5 millimoles of copper(II) sulfate has been added by the chemist to the flask.