anonymous
  • anonymous
A student adds 15.0 mL 2.00 M Acetic Acid and 15.0 mL 2.00 M NaOH. Determine the pH of the resulting solution. Ka HC2H3O2 = 1.80E-5
Chemistry
  • Stacey Warren - Expert brainly.com
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jamiebookeater
  • jamiebookeater
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anonymous
  • anonymous
This was my thought process. But it's saying that I have the answer incorrect by more than 10%
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aaronq
  • aaronq
you have to use the concentrations as equilibrium, after the reaction (f any) has occured. The NaOH will neutralize the acetic acid, and you'll be left with 0.03 moles of acetate in 30 mL. so can just use the Kb and an eq. expression to find the pH
anonymous
  • anonymous
@aaronq Okay, so would the equilibrium expression be Kc= [acetate] [OH-]/ [acetic acid]??

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aaronq
  • aaronq
nope, \(Acetate+H_2O\rightleftharpoons acetic~ acid+OH^-\) \(K_B=\dfrac{[acetic~ acid][OH^-]}{[acetate]}\)
aaronq
  • aaronq
oh, and \(\sf K_B=\dfrac{K_w}{K_A}\)

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