Mole ConceptHard
Question
A volume of 100 ml of M–NaCl solution, 100 ml of 2 M–MgCl2 solution and 300 ml of 4 M–Mg(NO3)2 solution is mixed together and the mixture is diluted to 2 L. Which of the following is/are the correct final concentration of ions?
Options
A.Na+ = 0.05 M
B.Mg2+ = 0.7 M
C.Cl– = 0.15 M
D.NO3 – = 1.2 M
Solution
For Na+: 2000 × $M_{\text{N}\text{a}^{+}}$ = 100 × 1 ⇒ $M_{\text{N}\text{a}^{+}}$= 0.05 M
For Mg2+: 2000 × $M_{\text{M}\text{g}^{\text{2+}}}$= 100 × 2 + 300 × 4
⇒ $M_{\text{M}\text{g}^{\text{2+}}}$ = 0.7 M.
For Cl–: 2000 × $M_{Cl^{-}}$= 100 × 1 + 100 × 2 × 2
⇒ $M_{Cl^{-}}$= 0.25 M
For$\text{N}\text{O}_{3}^{-}$: 2000 × $M_{\text{N}\text{O}_{3}^{-}}$= 300 × 4 × 2
⇒ $M_{\text{N}\text{O}_{3}^{-}}$= 1.2 M
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