1.0 M of HC2H3O2 =1.05 pH what would the pH be for 0.1 M and 0.01 M

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1.0 M of HC2H3O2 =1.05 pH what would the pH be for 0.1 M and 0.01 M

Chemistry
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i believe you need to figure out the pKa which is 4.74 and figure out how many [H+] ions there are THEN do -log10[H+]=pH
But for this problem it looks like it should decrease by a "tenfold"
acetic acid+h20===>acetate ion + h30+ I THINK YOU NEED TO DO "ICE"

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Other answers:

when you dissolve it, in which ions does it fall apart. If it for example acetate iuon + h30 then its 1:1 So fill in the concentration of the H+ es, you have the \[pH = -\log_{\left[ H+ \right]} \]

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