Answer:
[tex][SO_4^{-2}]=0.354M[/tex]
Explanation:
Hello,
In this case, we can write the ionization of salt and based on their concentration, apply the corresponding mole ratios as shown below:
- [tex]Na_2SO_4\rightarrow 2Na^++SO_4[/tex]: It has a 1:1 mole ratio to sulfate ion, therefore the concentration:
[tex]M_{SO_4^{2-}}=0.186 \frac{molNa_2SO_3}{L}* \frac{1molSO_4^{2-}}{1molNa_2SO_3} =0.186M[/tex]
- [tex]Al_2(SO_4)_3\rightarrow 2Al^{3+}+3SO_4^{2-}[/tex]: it has a 1:3 mole ratio to sulfate ion, therefore the concentration is:
[tex]M_{SO_4^{2-}}=0.0560 \frac{molAl_2(SO_4)_3}{L}* \frac{3molSO_4^{2-}}{1molAl_2(SO_4)_3} =0.168M[/tex]
Thus, the total concentration turns out:
[tex][SO_4^{-2}]=0.186M+0.168M=0.354M[/tex]
Best regards!
