In order to standardise a solution of hydrochloric acid, a
student titrated the solution against 20.00 mL aliquots of
a standard solution of sodium carbonate. Methyl orange
indicator was used to identify the end point of the reaction:
2HCl(aq) + Na2CO3(aq) → 2NaCl(aq) + H2O(l) + CO2(g)
The sodium carbonate solution had been prepared by
dissolving 1.236 g of anhydrous Na2CO3 in water and making
the solution up to 250.0 mL in a volumetric fl ask. The titres
recorded were 21.56 mL, 20.98 mL, 20.96 mL
and 21.03 mL.
a What value for the titre of hydrochloric acid solution
should the student use in the calculation of the acid
concentration? Explain your answer.
b What is the molarity of the sodium carbonate solution?
c Calculate the concentration of the HC l, in mol L−1.
with part c, i calculated the amount, in mol, of na2co3 and then i used the molar ratios to get twice the amount of na2co3 mol. After, i used what i found and plugged it into c= n/v, and got an answer as 1.11 something molar, which was incorrect. The answers did this:
c Step 1 From the equation, 2 mol of HCl reacts with 1 mol of Na2CO3 in the
Step 2 Calculate the concentration of hcl
n(HCl) = 2 x 0.04666 M x 0.02000 L
= 0.00186636 mol
c(HCl) = 0.00186636 mol/0.02099 L
= 0.088918 M
= 0.08892 M
help please!!