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
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
chem as level Watch
- Thread Starter
- 16-04-2016 00:20
- Official Rep
- 18-04-2016 01:40
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Just quoting in Puddles the Monkey so she can move the thread if needed
Spoiler:Show(Original post by Puddles the Monkey)