Chemistry Concentration and Solution Problem

Indicate the concentration of each ion present in the solution formed by mixing the following.

Assume that the volumes are additive.

(b) 44.0 mL of 0.265 M Na2SO4 and 31.0 mL of 0.150 M KCl
[Na+] ____ M
[K+] ____ M
[SO42-] ____ M
[Cl-] ____ M

(c) 3.60 g of KCl in 67.0 mL of 0.501 M CaCl2 solution
[K+] ______ M
[Ca2+] ______ M
[Cl-] ______ M

Answers with the explanation on how to find them would be very helpful. Thanks in advance.

(b)
Total volume: 44.0 mL + 31.0 mL = 75.0 mL
(44.0 mL) x (0.265 mol/L) x (2 mol Na{+} / 1 mol Na2SO4) / 75.0 mL = 0.311 M Na{+}
(31.0 mL) x (0.150 mol/L) x (1 mol K{+} / 1 mol KCl) / 75.0 mL = 0.0620 M K{+}
(44.0 mL) x (0.265 mol/L) x (1 mol SO4{2-} / 1 mol Na2SO4) / 75.0 mL = 0.155 M SO4{2-}
(31.0 mL) x (0.150 mol/L) x (1 mol Cl{-} / 1 mol KCl) / 75.0 mL = 0.0620 M Cl{-}

(c)
(3.60 g KCl) / (74.5515 g/mol) = 0.04829 mol K{+} and Cl{-}
The concentration of Ca{2+} doesn't change, so 0.501 M Ca{2+}
(0.04829 mol K{+}) / 0.0670 L = 0.721 M K{+}
[(0.04829 mol Cl{-}) + ((0.0670 L) x (0.501 mol/L) x (2 mol Cl{-} / 1 mol CaCl2))] /
(0.0670 L) = 1.72 M Cl{-}