The conversion of aqueous carbon dioxide to gaseous carbon dioxide is an endothermic reaction, so a weak acid with strong base neutralization can be simulated by adding heat to the reaction in Eq. 1. The addition of heat will promote the conversion of aqueous carbon dioxide to gaseous carbon dioxide in Eq. 3, thereby shifting the neutralization equilibrium nearly entirely to the right in accordance with Le Chatelier's principle and, thus, allowing a university-level weak acid/strong base titration to be conducted with more accessible household materials. By recording the pH as base is added, a titration curve can be created for acetic acid, from which the endpoint of the titration can be calculated by examining the point at which The concentration of acetic acid in the original vinegar analyte solution can be calculated using the concentration and volume of bicarbonate required to reach the endpoint of the titration. This calculated concentration of acetic acid can then be compared to the advertised value, which is approximately 1.0437M, assuming that the density of the acetic acid solution is 1.0446 g/mL at 25 o C. Precision is essential as there are limitations in the accuracy of household instruments.