# Chemistry

In aqueous solution, hydrochloric acid, HCl, and sodium carbonate, Na2CO3 react to
produce gaseous carbon dioxide, CO2, water, H2O and sodium chloride, NaCl. A 10.0 g impure
sample of Na2CO3 is dissolved completely in water; then treated with 3.00 mol L−1
HCl to evolve
1871 mL of gaseous CO2 at 25.0 °C and 100 kPa. The HCl solution is slowly added until the
evolution of gaseous CO2 is no longer observed.

a) Write down the balanced chemical equation for the reaction described above. Please include all
phases (i.e. aq, s, l, g, etc…).
b) What percent (by mass) of the impure sample is Na2CO3? Assume that the impure components
of the sample do not react with HCl.

1. 👍 0
2. 👎 0
3. 👁 336
1. Na2CO3(s) + 2HCl(aq) = H2O(l) + CO2(g) + 2NaCl(aq)

Use PV = nRT and solve for n = mols CO2 evolved at the conditions listed. Remember if you use kPa then R is 8.314. Remember T must be in kelvin.

Convert mols CO2 to mols Na2CO3 knowing that 1 mol CO2 requires 1 mol Na2CO3.

Convert mols Na2CO3 to grams. g = mols x molar mass

Then %Na2CO3 = (g Na2CO3/10g)*100 = ?

1. 👍 0
2. 👎 0

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