For our strong acid and base, hydrochloric acid and sodium hydroxide were chosen. Due to time restraints, our lab instructor told the class to perform only a single run of the reaction at each concentration. The experiment for the weak acid and base were conducted in Calorimeter One, and the experiment for the strong acid and base was conducted in Calorimeter Two. For the initial temperature, our team used the temperature of the solution already in the calorimeter before we added the second. Our team always placed the acid in the calorimeter first before adding the base. As seen in Tables 4 and 5, all of the results gleaned from the weak and strong acid base experiments were negative. Therefore, the results indicate that these particular acid base reactions released heat into their surroundings. The experiment itself further reinforced our interpretation of the results as both calorimeters became warmer as the reactions progressed. Thus, according to our experiments, reactions involving these two acid base reactions are exothermic processes. The reactions caused an increase in temperature in the surroundings by releasing heat from the system.As seen in Table 4, as the concentrations of the weak acid and base increased, so did the heat released by the reaction. One molar solutions gave off the least heat, and the six molar solutions gave off the most heat. Therefore, according to our results, the concentration did affect the amount of heat given off by the reaction in this experiment. The more concentrated the solutions of weak acid and base, the more heat is given off by the reaction. The same general trend is seen in Table 5 with the exception of the one molar solution of strong acid and base. The concentration does have an affect on the amount of heat released by the reaction. The one molar solution should have been the one that gave off the least heat, and the six molar solution should have given off the most he...
