What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution?

1.35M

0.450M*3=1.35M

Because the Na ion it was #of mol in the solution that has 3 Na ion and Molarity=mol/l then (mol*3) /l

Well, if we have a 0.450 M Na3PO4 solution, it means that for every 1 mole of Na3PO4, we have 3 moles of Na+. So, if we want to find the molar concentration of sodium ions, we just need to multiply the molarity of Na3PO4 by 3.

So, the molar concentration of sodium ions in a 0.450 M Na3PO4 solution is... drumroll please... 1.350 M! That's a whole lot of sodium swimming around in there. Don't go diving in that solution or you might turn into a pretzel!

To find the molar concentration of sodium ions (Na+) in a solution of Na3PO4, we need to consider the stoichiometry of the compound.

Na3PO4 is made up of three sodium ions (Na+) for every one phosphate ion (PO4^3-). Therefore, every mole of Na3PO4 will produce three moles of Na+ ions.

Given that the solution has a concentration of 0.450 M Na3PO4, it means there is 0.450 moles of Na3PO4 in every liter of the solution.

Since each mole of Na3PO4 produces three moles of Na+ ions, the molar concentration of Na+ ions is three times the concentration of Na3PO4.

So, the molar concentration of Na+ ions in a 0.450 M Na3PO4 solution is:

0.450 M Na3PO4 * 3 = 1.35 M Na+ ions.

Therefore, the molar concentration of sodium ions in a 0.450 M Na3PO4 solution is 1.35 M.

(Na3PO4) = 0.450 mols/L

There are three (3) Na^+ in 1 molecule of Na3PO4; therefore, (Na^+) must be 3x that.

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