Sodium Carbonic Acid Reaction Lab

Sodium Hydrogen Carbonate and Acetic Acid Reaction

Introduction

Not knowing whether calculations on a paper or an experiment are conducted correctly is one of the problems faced in chemistry. Luckily to ensure both calculations are correct, getting a one hundred percent yield is a necessity. “The actual yield of a product as a percentage of theoretical yield,”1 is how to determine the percent yield of a reaction. Actual yield is the amount, in grams, that a reaction actually produces while theoretical yield is the calculation, in grams, expected to be produced.

In any reaction, the Law of Conservation of Mass is applicable. This law ensures that the mass of a given reaction is the same in the beginning as in the end. To confirm that no mass

Afterwards, of the solution turning yellow, a white powder began to appear when all the water had disappeared. Now that, the solution had sixty- nine minutes to boil, the sodium hydrogen carbonate and the acetic acid produced sodium acetate.

Figure 1. The equipment setup for both days, the picture was taken at the end of day one.

Data

The overall data of the experiment is found in the calculation of percent yield. The data used in the equation were from the principle chemical equation of sodium hydrogen carbonate reacting with acetic acid to produce carbonic acid and sodium acetate. Only 0.05 moles of sodium hydrogen carbonate could to used so to determine the amount of grams to begin with the equation of converting moles to grams came into use. It was then found that 0.05 moles of sodium hydrogen carbonate is 4.2 grams. Grams = Moles x molar mass (2)

Converting moles into grams:

Grams= 0.05 grams NaHCO3x 83.978 grams 1 mol

Grams= 4.1989 grams NaHCO3 4.2 grams

Table 1 - The water level of the solution as x amount of minutes passed.

Time