Purpose
To experimentally determine the ideal mass of the sodium bicarbonate required to react with an acetic acid solution
Background

1NaHCO3 + 1HC2H2C2  1CO2 + 1 H2O + 1NaC2H3
Hypothesis
If the mole ratio of sodium bicarbonate to acetic acid solution stated in the balanced chemical equation is 1 to 1, then 1g of sodium bicarbonate will require exactly 14.9mL of acetic acid because 1.19 × 10-2 moles of the sodium bicarbonate requires 0.8 moles of acetic acid which has 1L, and 1L od any liquid is 1000mL of acetic acid.
Materials
1 Balloon
2 Flasks
Sodium Bicarbonate
Acetic Acid Solution
Graduated Cylinder
Measuring Tape
Calculator
Funnel
Weighing Balance
Weighing Boat
Procedures
1. Obtain all materials
2. Use the balance and the weighing boat to weigh out 1g of sodium bicarbonate. Subtract the weight of the weighing boat from the added weight of the sodium bicarbonate.
3. Use the funnel to pour the sodium bicarbonate into balloon. Lightly shake the balloon so that the all of the sodium bicarbonate gets inside balloon
4. Next measure out 10mL of acetic acid using the graduated cylinder
5. Pour the vinegar into flask
6. Wrap the opening of the balloon over top of the flask and spill the sodium bicarbonate into the flask with the balloon still wrapped around flask. Be careful to tip the sodium bicarbonate after the balloon is secured on the flask.
7. Wait until after reaction is over. Be sure to swirl the flask to make sure the reaction is over. ( no bubbles, or