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Chemistry
Solution Chemistry
Acids
At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
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-J
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At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
Thanks
Top answer:
Let's call acetic acid HAc. Then the ionization is HAc ==> H^+ + Ac^- We will call the initial concn
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At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
I am stuck. Thanks -J
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Answered above under needs help.
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At what initial concentration would a solution of acetic acid (ka=1.8x10^-5) be 2% ionized?
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The denominator is x-0.02x. That is 1.00x - 0.02x - 0.98x Think about it this way. 100%-2%=98% and
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so i had to calculate the pH of a 100ml solution of .10M acetic acid (ka=1.8x10(-5) I came out to 2.87. But then, they want the
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2.87 for pH of 0.1M HAc is right. For HCl + HAc first, what is the concn of the HCl added? If we
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Ac is acetate and HAc is acetic acid .......Ac + H^+ ==> HAc I....0.58...0........0.68
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Titration of 50.0 mL of acetic acid reaches equivalence after delivery of 22.5mL of standardized NaOH 0.21 M.
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