The aqueous solution contains 34.0% H3PO4 by weight and has a density of 1,209 g / ml. What is the molarity of this solution?
So in 100 g solution 34 g H3PO4 present
Molar mass of H3PO4 = (3×1) +(31×1) +(16×4) = 3+31+64 = 98 gmol-1
Mol of H3PO4 = 34\98 = 0.347 mol
100 g solution has a volume = 100\1.209 = 82.71 ml as volume = mass\ density
So molarity of solution
= (mol of solute)×1000 \(volume of solution in ml)
= (0.347×1000) \82.71
=4.19 M (ans)
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