Question
Asked Nov 8, 2019
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How many milliliters of a 0.1500-M solution of KOH will be required to titrate 40.00 mL of a 0.0656-M solution of H3PO4?
H3PO4(aq)+2KOH(aq)⟶K2HPO4(aq)+2H2O(l)

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Expert Answer

Step 1

The number of moles of H3PO4 is calculated as,

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No. of moles Molarity x Volume No. of moles 0.0656 (mol/L) x 40 x 103 (L) No. of moles 2.624 x 10-3 moles

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Step 2

Now, as per balanced chemical reaction, 1 mole H3PO4 reacts with 2 moles of KOH. Therefore,

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2.624 x 10-3 moles of H3PO4 will react with = 2 x 2.624 x 103 moles of KOH Hence, no. of moles of KOH= 5.248 x 103

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Step 3

Now, calculating the volu...

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No. of moles Molarity x Volume 5.248 x 10-3 0.15 x Volume Volume 0.03498 L Volume 34.98 mL

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