How Do You Calculate the pH of a Sodium Ethanoate Solution?

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The discussion revolves around calculating the pH of a 0.05 M solution of sodium ethanoate using the pKa of ethanoic acid, which is 4.75. The initial approach involves deriving the Ka from the pKa and assuming the concentration of acetate ions (CH3COO-) is equal to the sodium ethanoate concentration. However, there is a critique regarding the completeness of the explanation, emphasizing that multiple unknown concentrations exist in the system. Participants urge for clarity in distinguishing between ethanoate and ethanoic acid in the calculations and request the equations used to support the reasoning.
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Hi ppl. I have a question. I'm given the pka of ethanoic acid/ethanoate ions at 4.75 and i have to work out the ph of a 5*10^-2 moldm3 solution of sodium ethanoate. I worked it out by getting the Ka from 10^-4.75 and then saying that the concentration of Ch3COO- in the dissociation of ethanoic acid is also 5*10^-2 moldm3. Then i used the equation for the Ka to get the corresponding concentration of H+ ions in this dissociation and hence the ph, is this method of reasoning correct? Thanks, Joe
 
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The question itself seems to indicate an initial concentration of ethanoate, however, your discussion implies ethanoic acid? Please be more clear...
 

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