acid buffers - because without them the pH of our blood...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Miranda Pryor Chem 1310 A4 Acids, Bases, and Buffered Systems Conclusion: The main final result found in this experiment is that adding strong acids or bases to a buffered solution does not change the pH very much while adding them to water changes the pH drastically. Our results are accurate because we demonstrated the definition of a buffer. Also, we found that we could determine the K a of an unknown half- neutralized solution of weak acid. By finding the pH, we were easily able to calculate the H + ions which is the same as the K a in this instance. Post-Lab Questions: 1. Carbon dioxide might cause distilled water to have a pH that is less than 7. This is because it dissolves in water to form carbonic acid. CO 2 + H 2 O H 2 CO 3 2. Most of the buffers found in the body are in our blood. These buffers are important
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: because without them the pH of our blood would not be constant which could lead to acidosis or alkalosis and death. The phosphate buffer system is present inside cells in the human body. If the pH goes up in our cells, the pH is reduced by a reaction with H 2 PO 4-to use up the H+. H 2 PO 4-(aq) H + (aq) + HPO 4 2-(aq) In blood plasma, HCO 3-acts the same way as H 2 PO 4-to reduce the pH when it is too high. H 2 CO 3 (aq) H + (aq) + HCO 3-(aq) 3.pH=pKa+log([A-]/[HA]) 10.0 g 1 mol 82.03 g = .122 molanyhydroussodiumacetate .122 mol .1 L =1.22 Manyhydroussodiumacetate 4.74 + log(1.22 .1) = 5.8 4. Buffer capacity is the ability of a buffered solution to absorb protons or hydroxide ions without a significant change in pH....
View Full Document

This lab report was uploaded on 04/07/2008 for the course CHEM 1310 taught by Professor Cox during the Spring '08 term at Georgia Institute of Technology.

Ask a homework question - tutors are online