Calculate the solubility (common ion) buffered

  • Context: Chemistry 
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    Ion Solubility
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Discussion Overview

The discussion revolves around calculating the solubility of calcium oxalate (##\mathrm{CaC_2O_4}##) in a buffered solution, specifically considering the effects of common ions on solubility. Participants are exploring the initial steps and considerations necessary for solving the problem, including the use of an ICE table.

Discussion Character

  • Homework-related, Mathematical reasoning

Main Points Raised

  • One participant requests guidance on how to begin solving the problem.
  • Another participant suggests focusing on the concentration of the oxalate ion (##\mathrm{(COO^-)^2}##) as the relevant factor for the calculation.
  • A participant proposes setting up an ICE table for the dissociation of calcium oxalate and emphasizes the importance of the initial concentration of the dissociated ion.
  • One participant expresses doubt about the usefulness of the ICE table given that the initial concentration (I) is zero.
  • Another participant reiterates the importance of the oxalate ion concentration and questions the delay in progress.
  • A participant acknowledges a mistake in their earlier reasoning regarding the initial conditions of the problem.

Areas of Agreement / Disagreement

Participants appear to have differing views on the relevance and utility of the ICE table in this context, with some expressing uncertainty about starting conditions. The discussion remains unresolved regarding the best approach to take.

Contextual Notes

There are indications of missing assumptions regarding initial concentrations and the specific conditions of the buffered solution that may affect the solubility calculation.

il postino
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Homework Statement
Calculate the solubility of CaC2O4 in a 0.001M solution of Na2C2O4 buffered to pH equal to 4
Relevant Equations
Kps=(Ca+2).(C2O4-2)
Data:
##
pK_{ps} , pKa_{1} , pKa_{2}
##

Could you guide me to start solving?
Thank you!
 
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Hint: only concentration of (COO-)2 counts.
 
First, set up and ICE table for the chemical equation of ##\mathrm{CaC_2O_4}## and think about what the initial concentration of the relevant dissociated ion is.
 
Mayhem said:
set up and ICE table for the chemical equation of ##\mathrm{CaC_2O_4}##

Taking into account I is zero I don't think that will help much.
 
Borek said:
Hint: only concentration of (COO-)2 counts.
Which is in your Relevant Equation. So can start. Wonder what's taking?
 
Borek said:
Taking into account I is zero I don't think that will help much.
Borek said:
Taking into account I is zero I don't think that will help much.
Yes. My mistake. My brain completely skipped over important parts of the question.
 

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