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23 November, 14:27

What volume of a 0.25 m phosphoric acid solution is required to react completely with 1.0 l of 0.35 m sodium hydroxide?

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  1. 23 November, 15:36
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    The moles have to be equal. Always start with a balanced equation. This reaction is a double replacement.

    The basic equation is

    NaOH + H3PO4 = = = > Na3PO4 + HOH

    The balanced equation is.

    3NaOH + H3PO4 = = = > Na3PO4 + 3HOH

    moles of NaOH = moles of H3PO4

    mols of NaOH = molarity * Volume

    molarity = 0.35 mol/L

    Volume = 1.0 L

    moles NaOH = 0.35 * 1 = 0.35 mols

    Find the moles of H3PO4

    For every mol of H3PO4 used, you require 3 mols of NaOH

    3/1 = 0.35/x

    3x = 0.35

    x = 0.35/3

    x = 0.1167 moles of H3PO4 needed for this reaction.

    Now the volume needs to be calculated.

    n = 0.1167

    M = 0.25 mol/L

    V = ?

    Formula

    M = n/V

    V = n/M

    V = 0.1157/0.25

    V = 0.467 L

    Note: I merely copied the reaction given myself to the next line. I'm not copying from an outside source.
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