Problem: 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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Since the given reaction is already balanced, we can do a mole to mole comparison to calculate the number of moles of KOH to react with H3PO4 then calculate the volume of KOH solution needed.

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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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Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

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Based on our data, we think this problem is relevant for Professor Rexford's class at FSU.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.