Mass of the empty beaker98.9 g
Mass of the beaker + NaHCO399.4 g
Mass of the NaHCO30.5 g
Mass of the beaker + NaCl99.6 g
Mass of the NaCl0.7 g
Post Lab Questions
1.As I added the hydrochloric acid the solution turned a pale yellow color making the acid neutral. 2.Carbon dioxide was released during the chemical reaction. 3.It is evident that the sodium hydrogen carbonate underwent a chemical change because the beaker was warm and gaseous bubbles formed. 4.The resulting white powder in the beaker was crystallized during the reaction, forming the compound salt.
Analyze and Conclude
1.The product was different from the reactant because they all had a unique texture, color and also a different physical state. 2.To make sure that the white powder was all sodium chloride you would need to add more of hydrochloric acid to make sure that all of the sodium hydrogen carbonate was neutral and fully bonded. 3.The mass of the products was different from the mass of the original sodium hydrogen carbonate because the two elements bonded together, and some byproducts were created. Also, some of the moisture was evaporated away. 4.The experiment might have been affected if we added too much or too little of the hydrochloric acid to the beaker containing the sodium hydrogen carbonate.
Real World Chemistry
1.This chemical could relieve a stomach that contains excess acid because the sodium hydrogen carbonate would neutralize the acid, making it no longer hazardous to the body.