What is the Molarity of sodium ions in a 3.3 M solution of sodium phosphate?
the formula for sodium phosphate is ... Na3PO4
... three sodium atoms per molecule
How can I use that to find the molarity though?
To determine the molarity of sodium ions (Na+) in a solution of sodium phosphate, you need to consider the stoichiometry of the compound. Sodium phosphate (Na3PO4) contains three sodium ions for every one molecule of the compound.
To find the molarity of sodium ions, you can use the given molarity of sodium phosphate and the stoichiometry of the compound.
Step 1: Determine the number of moles of sodium phosphate in the 3.3 M solution.
Molarity is defined as moles of solute per liter of solution. Therefore, for a 3.3 M solution, you have 3.3 moles of sodium phosphate per liter.
Step 2: Use the stoichiometry of the compound to determine the number of moles of sodium ions in the solution.
Since sodium phosphate contains three sodium ions for every molecule of the compound, the number of moles of sodium ions is three times the number of moles of sodium phosphate.
Step 3: Calculate the molarity of sodium ions.
Divide the number of moles of sodium ions by the volume of the solution (in liters) to obtain the molarity of sodium ions.
Let's assume you have a 1-liter solution of sodium phosphate:
Number of moles of sodium phosphate = 3.3 moles
Number of moles of sodium ions = 3 x 3.3 moles = 9.9 moles
Molarity of sodium ions = 9.9 moles / 1 liter = 9.9 M
So, the molarity of sodium ions in a 3.3 M solution of sodium phosphate is 9.9 M.