How would this experiment change if the HCl was the standard solution and NaOH was the unknown?
How would this experiment change if the HCl was the standard solution and NaOH was the unknown?
Answer: If the experiment were to switch the roles of the solutions, with HCl becoming the standard solution and NaOH becoming the unknown solution, several changes in the experimental process would need to be made. Here are some key differences that would arise:
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Titration Process: The titration process would need to be adjusted accordingly. Initially, HCl would be placed in the burette, and NaOH solution would be in the conical flask. The endpoint of the titration would then be reached when the pink color of the phenolphthalein indicator turns colorless.
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Calculation of Molarity: Since HCl is the known standard solution in this scenario, its exact concentration would be used to determine the concentration of NaOH. The volume and concentration of HCl used during the titration would be crucial in calculating the molarity of the NaOH solution.
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Equivalence Point Calculation: The equivalence point in this case would be reached when stoichiometric amounts of HCl and NaOH have reacted. This point signifies that the moles of HCl are equal to the moles of NaOH, allowing for the calculation of the concentration of the NaOH solution.
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pH Change: The pH curve would show a different pattern compared to the traditional setup, reflecting the titration of NaOH with HCl. The equivalence point would occur at a pH lower than 7, indicative of the acidic nature of the resulting solution.
Switching the standard solution from NaOH to HCl requires adjustments in the experimental setup, calculations, and understanding of the chemical reactions involved in the titration process.