A student weighed 1.25 grams of NaHCO3 pre-weighed 50 mL beaker. In the fume hood, he slowly
added concentrated HCl to the beaker containing the NaHCO3. He added a total of 4.6 mL of
concentrated HCl. During the reaction, effervescence was observed due to carbon dioxide formation.
The water by-product was removed by heating the beaker and a white crystalline salt, NaCl, is left.
Lastly, he took the weight of the residue and the beaker after cooling to room temperature.
Mass of beaker (g): 28.27 g
Mass of NaHCO3 sample (g): 1.25 g
Mass of beaker and residue (g): 29.06 g
Volume of concentrated HCl (12moles/L) (ml): 4.6 mL
14. Write the balanced chemical equation for the reaction.
15. How many moles of NaHCO3 are in the sample?
16. How many moles of HCl are there in the sample?
17. How many moles of HCl are required to react completely with NaHCO3?
18. Which reagent is in excess and which reagent is limiting?
19. What is the theoretical yield of NaCl in grams?
20. What is the actual yield of NaCl in grams?
21. What is the percent yield of NaCl in grams?