Question

Calculate the molarity of each ion in solution after 2.0 litre of 3.0 M $AgN{O}_3$ is mixed with 3.0 litre of 1.0 M $BaC{l}_2$.

• A. Molarity of $B{a}^{2+}=1.2M;$ Molarity of $N{O}_3^{-}=1.2M$
• B. Molarity of $B{a}^{2+}=0.6M;$ Molarity of $N{O}_3^{-}=0.6M$
• C. Molarity of $B{a}^{2+}=0.6M;$ Molarity of $N{O}_3^{-}=1.2M$
• D. Molarity of $B{a}^{2+}=1.2M;$ Molarity of $N{O}_3^{-}=0.6M$

Answer 1

Answer: (C)

Molarity of $B{a}^{2+}=0.6M;$ Molarity of $N{O}_3^{-}=1.2M$

Total volume = 2+3 =5L

Moles of Ba${}^{2+}$ =3x1=3

Therefore, molarity of Ba${}^{2+}$ =$\frac{3}{5}$ =0.6M

Moles of NO${}_3^{-}$ =2x3=6

Molarity of NO${}_3$ =$\frac{6}{5}$=1.2M