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25 February, 04:01

What is the molarity of an aqueous phosphoric acid solution if 13.13 mL is completely neutralized by 19.64 mL of 0.09291 M NaOH? Collapse question part Part 1 Incorrect answer. Did you write the correct molecular formula for phosphoric acid? Write a balanced molecular equation for the reaction. Be sure to include the appropriate phases for all reagents and products.

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  1. 25 February, 04:26
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    The molarity of this solution is 0.0695 M

    Explanation:

    Step 1: The balanced equation

    H3PO4 (aq) + 2NaOH (aq) → Na2HPO4 (aq) + 2H2O (l)

    Step 2: Given data

    Volume of phosphoric acid (H3PO4) = 13.13 mL

    volume of NaOH = 19.64 mL

    Molarity of NaOH = 0.09291 M

    Step 3: Calculate moles of NaOH

    Number of moles = Molarity * volume

    Number of moles = 0.09291 M * 19.64 mL * 10^-3 L

    Number of moles = 0.001825 moles

    Step 4: Calculate moles of H3PO4

    For 2 moles of NaOH there is 1 mole of H3PO4 consumed to produce 1 mole Na2HPO4

    So for 0.001825 moles NaOH, there is consumed 0.001825/2 = 0.0009125 moles of H3PO4

    Step 5: Calculate molarity of H3PO4

    Molarity = number of moles / Volume

    Molarity = 0.0009125 moles / (13.13 * 10^-3L) = 0.0695 M

    The molarity of this solution is 0.0695 M
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