What mass of Uranium (in mg) is contained in 1ml of 4.55M (UO2)3(PO4)3 solution?

How do I solve this?
*all numbers are subscripts

To determine the mass of uranium in 1 mL of the given solution, we need to follow a step-by-step process:

1. Understand the chemical formula: (UO2)3(PO4)3 represents a compound containing uranium (U), oxygen (O), and phosphate (PO4) ions. The subscript 3 indicates that there are three units of this compound.

2. Calculate the molar mass: Find the molar mass of each element present in the compound. The molar mass of uranium is 238.03 g/mol, oxygen is 16.00 g/mol, and phosphorous is 30.97 g/mol. Since there are multiple units, multiply the molar mass of each element by the number of units given in the subscript. In this case, multiply the molar mass of (UO2)3 by 3 and (PO4)3 by 3.

(UO2)3 molar mass = 3 * (238.03 g/mol + 16.00 g/mol) = 3 * 254.03 g/mol = 762.09 g/mol

(PO4)3 molar mass = 3 * (30.97 g/mol + 4 * 16.00 g/mol) = 3 * 94.97 g/mol = 284.91 g/mol

3. Calculate the number of moles: The concentration of the solution is given as 4.55 M, which means there are 4.55 moles of (UO2)3(PO4)3 in 1 liter (or 1000 mL) of the solution. Since we want to find the mass in 1 mL, we need to calculate the number of moles in 1 mL. Divide the concentration by 1000 to convert from M to mol/mL.

Number of moles = 4.55 M / 1000 mL = 0.00455 mol/mL

4. Calculate the mass: Finally, multiply the number of moles by the molar mass of (UO2)3(PO4)3 to obtain the mass in grams. To convert grams to milligrams, multiply by 1000.

Mass = Number of moles * (UO2)3(PO4)3 molar mass

Mass = 0.00455 mol/mL * 762.09 g/mol * 1000 mg/g

Mass ≈ 3.47 mg (rounded to two decimal places)

Therefore, there is approximately 3.47 mg of uranium in 1 mL of the 4.55 M (UO2)3(PO4)3 solution.

How many mols do you have? That's M x L = mols.

There are 3 atoms U in 1 molecule of (UO2)3(PO4)3; therefore mols (UO2)3(PO4)3 x 3 = mols U
g U = mols U x atomic mass U.
Convert g to mg.