Discussion Overview
The discussion revolves around calculating the concentration of ethanoate ions in a solution of ethanoic acid using the acid dissociation constant (Ka). Participants explore the application of the ICE (Initial, Change, Equilibrium) method in this context, addressing challenges in setting up the calculations correctly.
Discussion Character
- Homework-related
- Mathematical reasoning
- Technical explanation
- Debate/contested
Main Points Raised
- One participant presents the problem of finding the concentration of ethanoate ions in a 0.18 mol/L solution of ethanoic acid, using Ka = 1.76 x 10-5.
- Another participant suggests that the ICE method is suitable and should work as expected.
- A participant attempts to set up the ICE table but arrives at a concentration of 0.1799999 mol/L, questioning the discrepancy with the expected answer of 1.8 x 10-3 mol/L.
- Another participant points out that the ICE table is incomplete and that the Ka expression is incorrectly set up, suggesting that the dissociation reaction should start with the undissociated substance as the reactant.
- A participant proposes a revised ICE table but struggles with the Ka expression, questioning the placement of products and reactants in the equation.
- There is confusion regarding the correct identification of products in the dissociation reaction, with participants discussing the roles of hydronium and acetate ions.
- Participants express uncertainty about the correct setup of the Ka expression and the ICE table conventions.
Areas of Agreement / Disagreement
Participants do not reach a consensus on the correct setup of the ICE table and the Ka expression. There are multiple competing views on how to approach the problem, and the discussion remains unresolved.
Contextual Notes
Participants highlight limitations in their understanding of the dissociation reaction and the proper conventions for setting up the ICE table and Ka expression. There are unresolved questions about the correct identification of products and the implications for the calculations.