Determination of a Ka Constant

Determination of a Ka Constant - Determination of a Ka...

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Determination of a K a Constant Lauren Tankesley and Megan Cobb-Young Purpose : Use the process of acid-base titration to neutralize an acid through titration of the base into the acid. The data gathered determines the equilibrium constant for a given acid. Theory : The equilibrium constant of a monoprotic weak acid can be determined by taking the concentration of the products and dividing it by the concentrations on the reactants. This value is notated by ‘K eq ’ and can give the K a – the acid dissociation constant – of a substance. Since equilibrium concentrations of the hydronium ions are so small, they are expressed with a ‘p’ since they are negative logarithms (log 10 ). In this particular experiment, the entirety of the initial acid is used and so rendering the log 10 ([A - ]/[HA])in the Henderson-Hasselbach equation as the value 0 which is therefore irrelevant: pH = pKa + log 10 ([A - ]/[HA]) With this said, the pH value determined from the graphed data represents the pKa from which one can derive the Ka of the acid in each trial. In each trial, a strong acid, NaOH, is used in a titration set-up to convert all the HA to A
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This note was uploaded on 04/02/2008 for the course CHEM 1212 taught by Professor Dockery during the Spring '08 term at Kennesaw.

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Determination of a Ka Constant - Determination of a Ka...

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