Answer:
[Co(H₂O)₆]²⁺ = 0.361 M
Explanation:
[CoCl₂ . 6H₂O] + 2Cl⁻ → [CoCl₄]²⁻ + 6H₂O
[Co(H₂O)₆]²⁺ + 4Cl⁻ → [CoCl₄]²⁻ + 6H₂O
[CoCl₄]²⁻ = 0.361 M ∴ [Co(H₂O)₆]²⁺ = 0.361 M
The equation shows that the concentration of [Co(H₂O)₆]²⁺ should be equal to the concentration of [CoCl₄]²⁻.
The concentration of [tex]\rm [Co(H_2O)_6^2^+][/tex] determined from the bottle in the lab has been 0.361 M.
The concentration of the solution can be determined as the moles of solute in a liter of solution.
The solution of [tex]\rm [CoCl_2.6\;H_2O][/tex] had the molar concentration of 0.71 M. The determined solution concentration of [tex]\rm [Co(H_2O)_6^2^+][/tex] has been 0.361. The formation of ions in the solution has been governed as:
[tex]\rm [CoCl_2.6\;H_2O]+2\;Cl^-\;\rightarrow\;[CoCl_4]^-\;+\;6\;H_2O\\\\Co(H_2O)_6^2^+\;+\;4\;Cl^-\;\rightarrow\;[CoCl_4]^-\;+\;6\;H_2O\\\\CoCl4^2^-=Co(H_2O)_6^2^+[/tex]
Thus, the concentration of the ions in the solution has been given as equivalent as:
[tex]\rm CoCl4^2^-=Co(H_2O)_6^2^+\\Co(H_2O)_6^2^+=0.361 \;M[/tex]
The concentration of [tex]\rm [Co(H_2O)_6^2^+][/tex] has been 0.361 M.
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