1. All the students separated themselves into groups of four or five.
2. Everyone grabbed and put on their safety googles.
3. The weighted scale was set up - making sure it was at 0.00 grams
4. The mass of the flask was recorded. (37.37g)
5. Using the scooper, 2.0+/- 0.2g of NaHCO3 was added directly to the flask.
Note :{ Contents inside the flask were white in color.}
6. The mass of both NaHCO3 and Flask was taken. (39.17g)
7. The amount of NaCHO3 alone was calculated. (1.8g)
8. Determined theoretical yield of NaCl by subtracting the mass of the flask by the mass of the flask and the NaHCO3. (1.3g)
9. The hypothesis was completed. “If 1.8 g of NaHCO3 is reacted with excess amount of HCl, then 1.3 g of NaCl will be produced.”
10. Using a graduated cylinder 31 mL of hydrochloric acid was obtained.
11.…show more content… Some of the HCl was poured into a beaker for easier access later.
12. Slowly the HCl was taken from the beaker drop by drop by use of a pipette and added to the NaHCO3, until the reaction was complete (bubbling stopped).
13. Flask was swirled after every 26th drop.
Note :{ Inside the flask was water, the contents were now clear in color.}
14. After reaction was complete the left over HCl from the beaker was poured back into the graduated cylinder to calculate the amount of HCl used (6mL) for the reaction to be completed.
15. MISTAKE Flask was put on a hot plate that was set at high.
16. Immediately the flask was taken off and let to cool.
17. On a hotplate set at medium, the flask was gently heated until the products began to
