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Final

CHEM 123 Final: Experiment 12B.docx

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Department
Chemistry
Course
CHEM 123
Professor
Tamara Kunz
Semester
Winter

Description
Experiment 12B: pH in Blood Abstract: The pH of a phosphate buffer solution was determined using a pH meter after the addition of NaOH or HCl, to show the affects of acidosis and alkalosis in blood. In order to lower the pH by one unit much more HCl (mL) is needed, than the amount of NaOH needed to raise the pH by one unit. Introduction: There are many medical cases of alkalosis and acidosis where, if not treated soon, may lead to death. In order to lower the blood pH (between 7.35 and 7.45), a treatment of injecting concentrated hydrochloric acid is used. The amount of hydrochloric acid to be injected is figured out from the total amount of excess base. Using concentrated hydrochloric acid to treat alkalosis is an effective way and it is a quick treatment method as well (Kwun 1983). In this experiment, the amount of HCl (or NaOH ) needed was determined in order to figure out how much (volume, mL) of each is required to change the buffer solution by one pH unit. When blood has alkalosis, a strong acid (HCl) is required to lower the pH to the desired amount. When the blood has acidosis, a strong base (NaOH) is required to increase the pH to the desired amount. The level of pH was determined by using a pH meter. Experimental Section: To prepare the phosphate buffer you use a beaker with 90mL of H P2 an4 use the pH probe to monitor the pH. Slowly add 1.0M NaOH until the pH reaches 7.45. Then pour content into a 250mL volumetric flask and add water until it reaches the line. For the buffer capacity use a pipet and add 25mL of buffer solution into a flask. Titrate this sample with 0.100M HCl until the pH drops by one unit. Use the microlab to record the change of pH as HCl is added drop by drop. Then titrate this sample with 0.100M NaOH until the pH rises by one unit. Use the microlab to record the change of pH as NaOH is added drop by drop. Next pipet another 25mL of buffer solution into a flask and add HCl dropwise until the pH lowers to 7.0. Then use the Restoration solution to raise the pH back to 7.45 and as this is being done it should be graphed on the computer (mircolab) as you add the restoration solution. Make sure to print out all three graphs. Results and Calculations: (D1) [H30]=Ka*[H2PO4]/[HPO4] 10^-7.45=6.3X10^-8*[RATIO] [RATIO]=0.5632 10^-7.45/6.3X10^-8=(0.563X+0.02)/(X-0.02) X=0.115m (0.5632X+X)*.25L/0.5M*1000ML/L =90mL (D2) ((0.020
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