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

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Discussion Overview

The discussion centers on determining the pH of a 0.15 M sodium acetate solution, focusing on the role of acetate as a weak base and its interaction with water. The context is primarily homework-related, involving theoretical and mathematical reasoning.

Discussion Character

  • Homework-related, Mathematical reasoning, Technical explanation

Main Points Raised

  • One participant suggests that since sodium acetate does not release hydrogen ions, the pH might be considered as that of pure water, which is 7.0.
  • Another participant counters this by stating that the pH of water is indeed affected by sodium acetate, as the acetate anion acts as a weak base.
  • A participant proposes a reaction involving acetate and water to determine the hydroxide ion concentration, indicating a potential method for calculating the pH.

Areas of Agreement / Disagreement

There is disagreement regarding whether the pH of the sodium acetate solution can be considered as 7.0. Some participants assert that the acetate anion affects the pH, while others question the initial assumption about the pH of water.

Contextual Notes

The discussion does not resolve the mathematical steps needed to calculate the pH, nor does it clarify the assumptions regarding the 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).

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

C2H3O2-+H2O <-> C2H3OOH + OH-?
 
Yes.

--
 
Thanks a lot!
 

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