Question

Sooo ml Chacool 0.300 M CH₂COOH Hot Chicoo + Moto 0.300M oh 20.00ml Nach CH₂COOH + NaOH → 0.500 TO ! xo.ooox 0.0200k Dois and 0.00600 0.06 0.00LOD 900x10 mal o Сан lint +0.706.00 6.000 Chiacto creat Ka L8x105 CH₂coot I (H) 90410 m 0.0700 L Hogy + CH₃CO5 g o brown mot +

Why is my professor using an ice table to solvs this titration problem? I seem to be confused with titrations and when to use an ice table with these kinds of problems. Iv seen similar problems being done without an ice table. Please break it down step by step explaing when and why we use ice tables to solve a titration question.

Answer 1

An ICE table is generally used when one wants to know the concentrations of components in a reaction at equilibrium when only given limited data such as initial concentrations and the reaction equilibrium constant. By solving for how each concentration is changed in a reaction (ICE table & quadratic formula), one is able to determine each concentration at equilibrium. Sometimes it's not necessary to us an ICE table, but it's helpful to better organize one's work.

Generally speaking, we should use an ICE table when the problem includes words like "determine molar concentrations in the mixture at equilibrium," "__ was placed into the reaction vessel," "initial," and "equilibrium concentrations."

You can also essentially use the ICE table in any acid base equilibrium problem to check your work. For example, when given the equilibrium concentrations of a product and asked to find Kc, you can use ICE to show how you found your Kc when you really don't need to.

Hope this helps!