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Titration - How to find the molar mass of an unknown diprotic acid? watch

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    When titrated with 25cm^3 of 0.05 M NaOH, it took 11.975 cm^3 of an unknown diprotic acid for a full neutralisation.

    The acid solution was made by dissolving 1.5g of solid acid in 250cm^3 of distilled water.

    The balanced equation for this reaction is 2NaOH + H2X -> Na2X + H2O.

    How can I work out the molar mass of the diprotic acid from this information? I know it is between 110 and 130
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    It is a fairly simple molar calc. using c =nv and n = m/Mr.

    Where are you struggling?
 
 
 
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