## ICE tables

Savannah Mance 4G
Posts: 107
Joined: Fri Aug 30, 2019 12:17 am

### ICE tables

How do you know when a question requires an ICE table? I know that an ICE table is only used when they don't give you the equilibrium initial concentration. But, will they tell you they're not the concentrations at equilibrium? How will the problem usually be worded for ones that require ICE tables?

AngieGarcia_4F
Posts: 120
Joined: Thu Jul 25, 2019 12:17 am

### Re: ICE tables

I think you use ICE tables when you're given K and an initial concentration and are asked to find a final concentration.

Andrew Liang 1I
Posts: 105
Joined: Fri Aug 30, 2019 12:18 am

### Re: ICE tables

You use ICE table when the question asks for the equilibrium composition of the reaction system. In other words, the system given in the question is usually not at an equilibrium so the question is basically asking us to find what is the concentration of each molecules when the system is finally at an equilibrium. ICE table allows us to find the final equilibrium composition.

vpena_1I
Posts: 109
Joined: Sat Aug 24, 2019 12:15 am

### Re: ICE tables

For problems that give you the molarity of a strong acid or base, you do not need an ICE table because you can assume the acid/base dissociated completely. If you are given only the molarity of a weak acid/base, you will need an ice table because you do not know the concentrations of the other solutions at equilibrium. Problems like these will also usually involve the use of Ka/Kb.

Tyler Angtuaco 1G
Posts: 130
Joined: Wed Sep 11, 2019 12:16 am

### Re: ICE tables

If the question does not state the values are at equilibrium, they are not. ICE tables are needed when the equilibrium values are not provided, but are not necessary if you know the equilibrium amount of one of the reactants or products. This is because you can use the stoichiometric ratios of the balanced reaction to determine the amount of change a reactant or product experiences from their initial amount, and then add or subtract to the initial amounts of reactants or products accordingly.