[no-stretch8180]

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?

[no-stretch8180]

i dont know hwo to do c and onwards

[AWK]

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.

[no-stretch8180]

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?

[AWK]

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?

[no-stretch8180]

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