Sodium Bicarbonate Formal Lab Report

Experimentally Finding Percent Mass of Carbon Dioxide in Sodium Bicarbonate

Formal Lab Report By: Tessa Amster

Lab Partners: Mia Cohoon, Ava Loebel, and Emma Murphy

Lab Dates: 02/09/2023, 02/13/2023

Lab Report Due: 03/08/2023

Purpose

The purpose of the lab was to determine the mass percent of carbon in sodium bicarbonate, also known as baking soda, by the means of measuring the mass of carbon dioxide gas produced in the chemical reaction.

Expected Results

The expected, or theoretical result was 52.39 percent composition of carbon dioxide in the equation. To find this value, the molar mass of carbon dioxide was calculated, being 44.01g, which was utilized in the formula to find percent composition, %CE = (gE/gT)×100, as the part,

The Theory of Conservation of mass states that matter can neither be created nor destroyed. In this experiment, this was utilized with the presence of the chemical equation and reaction that took place which released carbon dioxide. This theory forced us to use the balanced equation, NaHCO3(s) + CH3COOH(aq) → CH3COONa(aq) + H2O(l) + CO2(g), as well as assume the equal masses of our reactants and products. A french chemist, Joseph Louis Proust, observed that elements combine with one another in a definite mass

The expected results were found through the theoretical mass calculations, equalling 52.39%. The experimental mass was 30.%, meaning that the percent error was 42%. These are the results due to the law of consevation of mass, and law of definite proportions, as discussed previously. The law of conservation of mass was used in this experiment because the assumption was made that mass could not be lost in the reaction. The differing masses between the start and end of the reaction was due to the release of carbon dioxide, meaning that mass was not destroyed, but located beyond the confines the utilized beaker. The law of definite proportions was used in the ratios needed to determine the various calculations, specifically the percent composition of each element of acetic acid, and the calculations used in the findings of carbon dioxide. It implies that a precise quantity of each compound will be produced through the decomposistion of a compound. The experimental percent value was lower than the theoretical due to the circumstantial error. The required agitation of the solution is a potential cause of this mathematical error, meaning the solution should’ve been left sitting for longer before measurement. Potentially, the CO2 was still dissolved into the water, meaning the solution should have been swirled more to trigger the