In the Aspirin Titration Lab we calculated the number of moles of aspirin is each tablet, both low dose and regular strength aspirin, calculated the number of moles of NaOH is needed to titrate the aspirin and compared our predicted amount of NaOH to the amount actually used in the experiment. In this experiment we tested low dose and regular strength aspirin to figure out how much base (NaOH) would neutralize the aspirin. First grinded the aspirin tablet into a powder, added 5.0 mL of isopropanol, transferred it into a flask and swirled it to mix it all together. Then we added 25.0mL of DI water to the flask and 2 drops of phenolphthalein and swirled to mix. After that, we added NaOH into the burette and let it drip out into the flask, while we swirled it. We waited until the light pink color sat and stayed and recorded the final volume. We did that for both low dose and regular strength, recorded data for both. For low dose, our prediction was 4.5 mL of NaOH needed, but the actual volume of NaOH needed was 6.00mL. And for regular strength we predicted 18 mL of NaOH was going to be needed but the actual volume needed was 22.00 mL. Titration is the act of slowly adding one solution to a known volume of another solution of an unknown concentration until the substance reacts and becomes neutralized, often shown by color change. Titration is used to figure out the unknown concentration of an identified substance, volume measurements are a big part of titration.
Present Technology
Pharmacists can use many differeny ways to determine what the correct dosage of anything for a patient. They use various factors to determine the dosage, such as weight, age, height or functions of their organs such as kidneys. If a pharmacists is trying to look for a daily dose, they would probably multiply the factor and the dosing guidlines to figure out how much the patient is supposed to take daily.