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