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

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 =$\frac{2}{1}\times 0.25=0.50$ 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 =$\frac{1}{1}\times 0.25=0.25$ moles of $SO_4^{2-}$

Thus the concentration of $K^+$ and $SO_4^{2-}$ are 0.50 M and 0.25 M respectively.