Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: no-stretch8180 on January 12, 2021, 09:30:33 AM
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2.13 g of a carbonate M2CO3 was dissolved in water and made up to 100 cm3
in
a volumetric flask. 10.0 cm3 of this solution required 18.50 cm3 of 0.100 mol dm−3
hydrochloric acid for neutralisation.
The equation below represents the reaction between the acid and the carbonate:
2HCl(aq) M2CO3(aq) → 2MCl(aq) H2O(l) CO2(g)
a Calculate the amount in moles of HCl needed to neutralise 10.0 cm3 of the
carbonate solution.
b Using the equation above, write down the amount in moles of M2CO3 used
in the titration.
c Calculate the amount in moles of M2CO3 in 100 cm3 of the carbonate
solution.
d Calculate the molar mass of M2CO3
e Calculate the relative atomic mass of M. Give your answer to one decimal
place.
f Use the Periodic Table to identify M in the formula M2CO3
HOW DO I DO C?
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i dont know hwo to do c and onwards
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If you can calculate the moles in 10 cm3, why can't you calculate it in 100 cm3?
There is a simple mathematical relationship between the mass of a chemical compound and the number of moles in a sample.
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If you can calculate the moles in 10 cm3, why can't you calculate it in 100 cm3?
There is a simple mathematical relationship between the mass of a chemical compound and the number of moles in a sample.
so i did 0.1 x 0.1 = 0.01 is this right?
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If you can calculate the moles in 10 cm3, why can't you calculate it in 100 cm3?
There is a simple mathematical relationship between the mass of a chemical compound and the number of moles in a sample.
so i did 0.1 x 0.1 = 0.01 is this right?
And what do the reaction stoichiometry and titration say?
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If you can calculate the moles in 10 cm3, why can't you calculate it in 100 cm3?
There is a simple mathematical relationship between the mass of a chemical compound and the number of moles in a sample.
so i did 0.1 x 0.1 = 0.01 is this right?
And what do the reaction stoichiometry and titration say?
theres a 2:1 ratio for HCL:m2co3