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# pKaLab - Calculating the pKa of an Acid Using the...

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Unformatted text preview: Calculating the pKa of an Acid Using the Half-Neutralization Method Introduction Acid-base reactions involve neutralization between an acid and a base. The ability of an acid to donate its proton is dependent on the strength of the acid. Strong acids will completely dissociate – the concentration of [H + ] in a 0.1 M solution of HCl is 0.1 M. However, weak acids only partially dissociate and will only form a smaller concentration of H + relative to the HA present. As with any equilibrium constant for any reaction, the constant is a ratio of the concentration of the products to the concentration of the reactants. For the weak acid reaction HA ( aq ) H + ( aq ) + A- ( aq ) the equilibrium constant K a is K a = [H + ][A- ]/[HA] The value of K a lets us determine whether the equilibrium lies to the left or to the right, and thus the strength of the acid. If you take a weak acid and titrate it with a strong base such as NaOH, partway through the titration, you will reach what is known as the half-equivalence point . This is the point where the concentration of acid and deprotonated acid are equal to each other – also equal to half an equivalent of base having been added (by definition, at the endpoint of...
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pKaLab - Calculating the pKa of an Acid Using the...

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