Calculations involving K

True or False: You can use initial concentrations to directly solve for K_c

True or False: You can use initial concentrations to directly solve for K_c

false

• must be converted to equilibrium concentrations

In terms of initial concentrations, what table is used? What conditions must be satisfied to use this table?

1. an ICE table

2. the molecules must be aqueous or gaseous

What does ICE stand for?

I = initial concentration(s)

C = change in concentrations of reactants(-)/products(+)

E = equilibrium concentrations of reactants/products

What does x stand for in ICE tables?

the change of concentration

How can you solve questions using an ICE table?

1. Write the balanced equation

2. Use an ICE table to get equilibrium concentrations

3. Solve for x

4. Solve for all equilibrium concentrations and solve for K

What is considered a very small value for K_c? What are favoured as a result? What are negligible? Especially applicable to?

1. 10^-3 or less

2. reactants are favoured

3. ∆ [R]

4. weak acids and bases which experience very little ionization

   1. most species remain in molecular form