Calculating Concentrations in a Buffer Solution

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To calculate the concentrations of ethanoic acid and ethanoate ions in a buffer solution made from 50 mL of 0.05M ethanoic acid and 50 mL of 0.05M sodium ethanoate, simple dilution must be considered. When the two solutions are mixed, the final volume becomes 100 mL, which affects the concentrations. The initial concentrations of both components are halved due to the dilution, resulting in 0.025M for both ethanoic acid and ethanoate ions. The Henderson-Hasselbalch equation is not necessary for this calculation, as the focus should be on the dilution effect. Understanding the dilution principle is key to accurately determining the final concentrations in the buffer solution.
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Homework Statement [/b]
A buffer solution was made using 50mL of 0.05M of ethanoic acid and 50mL 0.05 of sodium ethanoate. The question asks what is the concentration of ethanoic acid and ethanoate ions in the buffer solution. I assumed it would be 0.05M but when I asked for help I was told to work out the ethanaote ions by using Henderson-Hasselbalch equation first then work out the acid concentration. The pKa value of ethanoic acid is 4.76. I guess its something to do with the fact pH=pKa maybe, then find out the [H+]? so 10*-4.76 as my concentration
 
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No need for HH equation here, but once you mix 50 mL with 50 mL final concentrations are not 0.05M. Think simple dilution.
 
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