What are the concentrations of HA and A- at this point in concentration?

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Discussion Overview

The discussion revolves around calculating the concentrations of a weak monoprotic acid (HA) and its conjugate base (A-) during a titration process. Participants are exploring the necessary steps and equations to determine these concentrations based on given quantities of acid and base.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant reiterates the problem statement and asks where to start, indicating a need for guidance on the approach.
  • Another participant emphasizes the importance of showing attempts at solving the question to receive help, referencing forum policy.
  • A different participant suggests using the ion product constant of water (Kw) and provides a method to calculate the concentrations of HA and A- by first determining the concentration of the weak acid and the strong base separately.
  • This participant also mentions using the relationship Kw = [H+] [OH-] to find the concentration of H+ ions after calculating the concentration of OH- from the NaOH solution.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the specific steps to take, as some are seeking clarification while others propose methods. The discussion remains unresolved regarding the exact approach to calculate the concentrations of HA and A-.

Contextual Notes

Participants have not provided specific assumptions or definitions that may affect the calculations, and there are unresolved mathematical steps in the proposed methods.

Complexity
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Homework Statement



0.00116 moles of a weak monoprotic acid was dissolved in 25.0 mL in water. This solution was titrated with 10.0 mL of 0.0633 M NaOH. What are the concentrations of HA and A- at this point in concentration?


Homework Equations





The Attempt at a Solution

 
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Complexity said:

Homework Statement



0.00116 moles of a weak monoprotic acid was dissolved in 25.0 mL in water. This solution was titrated with 10.0 mL of 0.0633 M NaOH. What are the concentrations of HA and A- at this point in concentration?


Homework Equations





The Attempt at a Solution


Where do I start?
 
Reaction equation won't hurt.

You have to show your attempts at solving the question to receive help. This is a forum policy.
 
Complexity said:

Homework Statement



0.00116 moles of a weak monoprotic acid was dissolved in 25.0 mL in water. This solution was titrated with 10.0 mL of 0.0633 M NaOH. What are the concentrations of HA and A- at this point in concentration?


Homework Equations





The Attempt at a Solution


Maybe you do it using Kw ...
Find the concentration of the weak acid using c= n/v where c is concentration, n is moles and v is volume...
then find the concentration of base using the same formula... since the base is strong , OH concentration is the same as the base itself.i.e.NaOH ...

Now use,
Kw = [H+] [OH-]
use Kw as 10^-14
and conc of OH u calculated earlier..
find conc of H+ ions...the rest is simple...
 

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