Question

3.66 g of MgSO₄ is placed into 100.0 mL of water. What is the molarity of the MgSO₄ solution?

A) 0.366 M
B) 0.183 M
C) 0.366 mol/L
D) 0.183 mol/L

Answer 1

The molarity of the MgSO₄ solution is calculated by dividing the moles of MgSO₄ by the volume of the solution in liters. After calculating the moles based on the given mass and molar mass of MgSO₄, the molarity is found to be 0.304 M, which does not match any of the provided options.

Step-by-step explanation:

To calculate the molarity of the MgSO₄ solution, you would use the formula:

Molarity (M) = moles of solute / liters of solution

First, we need to find the moles of MgSO₄. The molar mass of MgSO₄ is approximately 120.37 g/mol (24.305 + 32.065 + (16.00 x 4)). Therefore:

moles of MgSO₄ = 3.66 g / 120.37 g/mol = 0.0304 moles

Now, since we have 100.0 mL of solution, which is equivalent to 0.1000 L, we can find the molarity:

Molarity = 0.0304 moles / 0.1000 L = 0.304 M

This molarity needs to be converted to a matching answer from the options given. Since none of the answers match, it seems there might be a typo. Yet, the correct process has been detailed above.