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    The student adds a lump of limestone with mass 0.13 g to 25.00 cm3 of 0.100 mol dm–3 hydrochloric
    acid and stirs until the reaction is finished. The solution is then filtered.
    The excess acid in the filtered solution reacts with 7.00 cm3
    of 0.100 mol dm–3 sodium hydroxide.
    The equations for the reactions are:
    CaCO3 + 2HCl → CaCl2 + CO2 + H2O
    HCl + NaOH → NaCl + H2O
    now the question is The student realises that the percentage of calcium carbonate should be given to two significant
    figures.
    Suggest how the student might vary the method, using the same apparatus, to get a result that could
    be accurately reported to three significant figures
    can someone explain this to me
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    Sorry you've not had any responses about this. Are you sure you've posted in the right place? Here's a link to our subject forum which should help get you more responses if you post there.

    You can also find the Exam Thread list for A-levels here and GCSE here. :dumbells:


    Just quoting in Puddles the Monkey so she can move the thread if needed
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