What is the pH of a 0.15M Sodium Acetate Solution?

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The pH of a 0.15 M sodium acetate solution can be determined by recognizing that sodium acetate dissociates to produce acetate ions, which act as a weak base. The acetate anion reacts with water to form acetic acid and hydroxide ions, affecting the pH. The equilibrium expression can be used to calculate the concentration of hydroxide ions, which is necessary for determining the pH. The pH of pure water is not applicable here since the acetate alters the solution's acidity. Therefore, the pH must be calculated based on the weak base behavior of acetate in solution.
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Homework Statement



Determine the pH of0.15 M solution of sodium acetate, ka = 1.8 x 10^-5




The Attempt at a Solution



Since there are no hydrogen ions that dissolve from sodium acetate, would I use the pH of water =7.0? Is the pH of water even affected by sodium acetate?
 
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flyers said:
would I use the pH of water =7.0?

No.

Is the pH of water even affected by sodium acetate?

Yes.

Acetate anion is a weak base (conjugate base of acetic acid).

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OK, so the OH concentration can be found by this reaction

C2H3O2-+H2O <-> C2H3OOH + OH-?
 
Yes.

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Thanks a lot!
 

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