Plop, Plop, Fizz, Fizz, - Ms. Scholle



Plop, Plop, Fizz, Fizz,

Limiting Reagent and Determination of NaHCO3

in Alka Seltzer Tablets

Introduction

The extent of a chemical reaction is determined by the amount of reacting materials, or reactants, present in the reacting system. Reagents are generally not mixed in exact amounts needed for the reaction to take place, there is usually one of the reacting materials added in excess. The excess reagent, usually a non-critical reagent or an inexpensive material, is used to insure that all of the critical reagent is used up so that there will be a maximum amount of product formed. Also, an excess of one reactant can cause the overall reaction to take place at a faster rate. Once the critical reactant is used up, the reaction will stop. That critical reactant is called the limiting reagent, that is, it is the reactant in the chemical reaction that is used up first.

Alka Seltzer, and similar over-the-counter combination antacid and pain relief medications, contain aspirin

(acetylsalicylic acid), citric acid, and NaHCO3 as the active ingredients. This medication is designed to be

taken by dissolving it in water before ingesting. The carbon dioxide, from the reaction, escapes into the

atmosphere and results in a weight loss from the total mass of the reactants. Using the loss in mass, one can

calculate the amount of sodium bicarbonate reacted, and determine the percent by mass of NaHCO3 contained in Alka Seltzer tablets.

In this experiment, the Alka Seltzer tablets will be reacted with differing amounts of acetic acid, HC2H3O2, to produce the carbon dioxide. From the data, and graph of the data, the mass of the sodium bicarbonate in the Alka Seltzer tablets can be calculated, and the identity of the limiting reagent can be determined.

Materials – per partnership

2 tablets, Alka Seltzer Tablets

Acetic acid - 4.5 to 5% (vinegar)

2 - 250 mL beakers

10 mL graduated cylinder

50 mL graduated cylinder

glass stirring rod

PROCEDURE

1. Record the amount of vinegar you and your partner will be testing here: ________mL & _______mL and in data Table 1.

2. Measure the first amount of vinegar using a graduated cylinder and pour into a 250 mL beaker.

3. Measure the amount of water you would need to add to make the total liquid volume = 40.0 mL using a graduated cylinder and pour into the same 250mL beaker; stir.

4. Record the mL of water in data Table 1.

5. Mass the beaker w/liquid and record in data Table 1.

6. Mass an Alka Seltzer tablet and record in data Table 1.

7. Place the Alka Seltzer tablet into the 250 mL beaker w/water.

8. When the bubbling has stoppped, stir the solution to make sure the tablet has completely dissolved and to remove any visible bubbles of carbon dioxide. Gently tap the stirring rod against the inside of the beaker to remove any drops of liquid.

9. Mass the beaker and its contents. Record the mass and record in Table 1.

10. Dispose of the solution in the beaker down the sink.

11. Wash the beaker w/alconox and rinse it with distilled water.

12. Repeat the experiment using the other amount of acetic acid (vinegar) you were assigned and the corresponding water mL to equal 40.0 mL of liquid.

PRE-LAB:

1. Sodium bicarbonate reacts with acetic acid to produce sodium acetate, carbon dioxide, and water. Write the complete balanced equation below.

2. What is the mole ratio between all compounds of this reaction?

3. Can you tell by the balanced equation what the limiting reactant is? Why/Why not?

4. For the experiment the total volume of the liquid must equal 40.0 mL for each trial. Fill in the following data table to indicate the amount of water to be added to the vinegar.

|Volume of Vinegar |Volume of water (mL)|

|(mL) | |

|0.0 | |

|5.0 | |

|10.0 | |

|25.0 | |

|30.0 | |

5. Use the following data to answer the questions…

|mL Vinegar |mL Water |Mass liquid in |Mass Alka Seltzer |Mass beaker & |Mass of beaker & |Mass of CO2 (loss |

| | |beaker (g) |Tablets (g) |contents before |contents after |of mass) (g) |

| | | | |rxn. (g) |rxn. (g) | |

| | | |B |A + B |C |(A + B) – C |

| | |A | | | | |

|5.0 |35.0 |145.0 |3.23 |148.23 |147.60 |0.63 |

|20.0 |20.0 |148.0 |3.27 | |150.12 | |

a. Fill in the missing data from the second trial

b. To determine the mass of Na HCO3 in the alka seltzer tablet, you must use a stoichiometric calculation in which you start with the mass of CO2 produced and determine the amount of NaHCO3 that must have reacted to produce that. Find the mass of NaHCO3 in each tablet given in the data table above.

Trial 1:

Trial 2:

6. The % NaHCO3 in each alka seltzer tablet can be determined by dividing the gNaHCO3 in the tablet by the total mass of the tablet. Find the % NaHCO3 for each tablet in the data table above.

Trial 1:

Trial 2:

Data Table 1: Partner Data

|Exp. |Volume of Vinegar |Volume of Water (mL) |Mass of beaker & |Mass of Alka |Total mass of beaker and |

|# |(mL) | |liquid (g) |Seltzer tablet |contents before rxn. (g) |

| | | | |(g) |(A + B) |

| | | | | | |

| | | |A |B | |

|1 |0.0 mL | | | | |

|2 |5.0 | | | | |

|3 |10.0 | | | | |

|4 |15.0 | | | | |

|5 |20.0 | | | | |

|6 |25.0 | | | | |

|7 |30.0 | | | | |

|8 |35.0 | | | | |

|9 |40.0 | | | | |

Data Table 3: Class Average Data for Graph

Calculcations: Show all of your calculations used to complete Data Table 1.

Trial 1:

Trial 2:

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