Question

Write the dissociation equation for, and give the proper concentrations for a 0.25M K2SO4 solution

Answer 1

Answer:
`K_2SO_4\rightarrow 2K^++SO_4^(2-)`

concentration of
`K^+` = 0.50 M

concentration of
`SO_4^(2-)` = 0.25 M

Step-by-step explanation:

The dissociation equation of
`K_2SO_4` is:

`K_2SO_4\rightarrow 2K^++SO_4^(2-)`

According to stoichiometry:

1 mole of
`K_2SO_4` gives 2 moles of
`K^+`

Thus 0.25 moles of
`K_2SO_4` gives =
`(2)/(1)* 0.25=0.50` moles of
`K^+`

Similarly,

1 mole of
`K_2SO_4` gives = 1 mole of
`SO_4^(2-)`

Thus 0.25 moles of
`K_2SO_4` gives =
`(1)/(1)* 0.25=0.25` moles of
`SO_4^(2-)`

Thus the concentration of
`K^+` and
`SO_4^(2-)` are 0.50 M and 0.25 M respectively.