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Stoichiometric Calculations

A sample of ...

Question

A sample of $P_{2} O_{6}$ contains some $H_{3} P O_{4}$ impurity. A $0.405$ g sample is reacted with water ( $P_{2} O_{5} + 3 H_{2} O \to 2 H_{3} P O_{4}$ ), and the resulting solution is titrated with $0.25 M$ $N a O H$ requiring $42.5$ mL (upto $N a_{2} H P O_{4}$ ). The percentage purity of $H_{3} P O_{4}$ as nearest integer is :

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Solution

The number of millimoles of NaOH $= 0.25 \times 42.5 = 10.625$ millimoles.
The number of millimoles of phosphoric acid $0.5 \times 10.625 = 5.3125$ millimoles.
The number of millmoles of phosphorus pentoxide $= 0.5 \times 5.3125 = 2.65$ millimoles.
Mass of phosphorus pentoxide $= 2.65 \times 10^{- 3} \times 142 = 0.37718$ g.
So, $%$ purity is $25$ .

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