An aqueous solution of sodium phosphate, Na3PO4 is 20.0% Na3PO4 by mass, and has a density of 1.22 g mL−1. What is the molar concentration of sodium ions (Na+) in the solution?Molar masses: Na3PO4 163.94 g mol−1; H2O 18.016 g mol−1
Question
An aqueous solution of sodium phosphate, Na3PO4 is 20.0% Na3PO4 by mass, and has a density of 1.22 g mL−1. What is the molar concentration of sodium ions (Na+) in the solution?Molar masses: Na3PO4 163.94 g mol−1; H2O 18.016 g mol−1
Solution
Sure, here are the steps to calculate the molar concentration of sodium ions (Na+) in the solution:
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Calculate the mass of Na3PO4 in 1 mL of solution: 20.0% of 1.22 g is 0.244 g.
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Convert the mass of Na3PO4 to moles: 0.244 g / 163.94 g/mol = 0.00149 mol.
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Since each formula unit of Na3PO4 contains three Na+ ions, the number of moles of Na+ is three times the number of moles of Na3PO4: 0.00149 mol * 3 = 0.00447 mol.
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The molar concentration of Na+ is the number of moles per liter. Since we calculated the number of moles in 1 mL, we need to multiply by 1000 to convert to liters: 0.00447 mol * 1000 = 4.47 mol/L.
So, the molar concentration of sodium ions (Na+) in the solution is 4.47 mol/L.
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