The Neutrality of NaCl: Comparing H+ and Ac-

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Discussion Overview

The discussion revolves around the neutrality of sodium chloride (NaCl) in solution and the behavior of hydrogen ions (H+) in relation to acetic acid (HAc) and acetate ions (Ac-). Participants explore the differences in pH behavior between solutions of NaCl and sodium acetate (NaAc), focusing on the implications of strong versus weak acids.

Discussion Character

  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • Some participants note that NaCl is concluded to be neither acidic nor basic, with no change in pH.
  • There is a question about why the pH of a solution of NaAc is treated differently, with H+ combining with Ac- to form HAc.
  • One participant points out the distinction between hydrochloric acid (HCl) as a strong acid and acetic acid as a weak acid.
  • Another participant suggests that Cl- ions would not react with H+ in a way that changes their state, while H+ would react with Ac- to form HAc, which remains partially undissociated.
  • A correction is made regarding terminology, specifying "undissociated" rather than "undissolved."

Areas of Agreement / Disagreement

Participants express differing views on the behavior of ions in solutions of NaCl and NaAc, indicating that the discussion remains unresolved regarding the implications of these behaviors on pH.

Contextual Notes

Participants have not fully explored the assumptions underlying the behavior of strong versus weak acids in solution, nor have they resolved the implications of these behaviors on pH changes.

Kqwert
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Homework Statement
Hello,

I have two similar tasks here, but I don't really see any similarities in how they are "treated".

First question:

Calculate the pH of 0.01M NaCl.


Second question:

Find pH if you dissolve 0.2 mol NaAc and 0.1 mol HCl in water.
Relevant Equations
.
First question:
Here they just conclude that NaCl is neither acidic or basic, and that pH is unchanged.Second question:
Here I thought that the pH would just be the concentration of HCl, as NaAc is a salt, but in the solution they instead say that H+ will combine with Ac- to form HAc. Why is these two questions different? To me they seem very similar...
 
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Acetic acid is a weak acid, hydrochloric acid is a strong acid.
 
Thanks! so Cl- reacting with H+ would just result in Cl- and H+ ions back again, as HCl is a strong acid? Where as for the second case H+ will react with Ac- to form, and some of the HAc will remain undissolved undissociated as it is a weak acid?
 
Last edited:
Undissociated, not undissolved.
 
Thank you! I edited my post, is it correct now?
 
Yes
 
Correct, but you have not pushed anything as far as answering the questions.
 

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