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    Okay with my chemistry coursework I am hydrolysing esters using different acid catalysts.
    Comparing the initial rates of reactions with 2.0M Sulphuric acid and Hydrochloric acids, I was expecting the Sulphuric to result in double the rate, due to it being a di-protonator, but they both give the same rate. Does anyone have any ideas as to why?
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    (Original post by insiniac)
    Okay with my chemistry coursework I am hydrolysing esters using different acid catalysts.
    Comparing the initial rates of reactions with 2.0M Sulphuric acid and Hydrochloric acids, I was expecting the Sulphuric to result in double the rate, due to it being a di-protonator, but they both give the same rate. Does anyone have any ideas as to why?
    you gotta deduce your investigation based on your result. then you have to suggest reasons based on other literature evidence.

    a few key terms/phrases to read;
    1) order of reaction
    2) rate of reaction relation with orders of the reactants
    3) hydrolysis mechanism(perhaps)
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    (Original post by insiniac)
    Okay with my chemistry coursework I am hydrolysing esters using different acid catalysts.
    Comparing the initial rates of reactions with 2.0M Sulphuric acid and Hydrochloric acids, I was expecting the Sulphuric to result in double the rate, due to it being a di-protonator, but they both give the same rate. Does anyone have any ideas as to why?
    I'm not sure if this helps but.. Sulphuric acid doesn't completely dissociate and wont give double the concentration of H+ that comes from HCl. The second ionisation is suppressed by the hydrogen ions so HsO4- --> H+ + SO42- happens only a slight amount.

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