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Unformatted text preview: GSI- Beck Jacob Ziperstein Determination of the Molarity of a Strong Acid DON’T I NCLUDE HYPOT HESES REME MBER TO SITE ALL SOURCES DON’T HAVE T HE F IRST L I NE I N T HE I N TRO ADD RESULTS TO CONCLUSION Fix bibliography Change first sentence of methods. Don’t need all of the methods section Abstract: The purpose of this experiment was to successfully perform titrations in order to figure out the concentration of a solution of diluted Hydrochloric acid (HCl). The secondary objective of this lab was to master the techniques of titration. I performed three separate titrations, all of which were reasonably precise, but not accurate. My percent differences were 2.54%, 1.42%, and 1.17% respectively. The biggest source of error was that I unintentionally titrated too quickly, allowing too many milliliters of the HCl to be transferred to rapidly. The average between my three trials was .1976 M of HCl. I ntroduction The primary skill that was needed do successfully complete this lab was being able to perform a titration accurately. Titration is a technique that is commonly used when there is a solution of a known concentration, and one is t rying to determine the concentration of an unknown solution. The known solution is called the titrate, and is added via a buret to a “quantity of the analyte (the unknown solution) until the reaction is complete.” (1) In this particular lab, we GSI- Beck Jacob Ziperstein Determination of the Molarity of a Strong Acid conducted an Acid/Base titration, t rying to find the neutralized balance between the two solutions. Knowing the specific volume of the added titrate allowed us to determine the exact concentration of the unknown solution. An indicator, in this case bromocresol green, is generally used to signal the end of the reaction, known as the end-point. (The diagram to the right shows the different colors bromocresol green turns to at different pH levels). The end- point is also known as the equivalence point - when the two solutions contain the same number of moles. The indicator is vital in determining when you have completed the reaction. The color of the flask will change from blue to green to yellow as HCl is added. To determine how well you titrated, simply green to yellow as HCl is added....
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This note was uploaded on 09/04/2010 for the course CHEM 10966 taught by Professor Vollhardt during the Spring '10 term at Berkeley.
- Spring '10