Question

Solutions are made by dissolving .650g of each of the compounds below to make 1.9L of aqueous solution. What is the concentration of the chloride ions,[Cl-], in each solution?

CH2Cl2       LiCl      NiCl2    Ba(ClO2)2

[Cl-] in .65 g of CH2Cl2 in a 1.9 L solution= ? M

[Cl-] in .65 g of LiCl in a 1.9 L solution= ? M

[Cl-] in .65 g of NiCl2 in a 1.9 L solution= ? M

[Cl-] in .65 g of Ba(ClO2)2 in a 1.9 L solution= ? M

Answer 1

Solutions are made by dissolving 0.650g of each of the compounds below to make 1.9 L of aqueous solution. The concentration of the chloride ions,[Cl-], in each solution are:

[Cl-] in 0.65 g of CH2Cl2(it will not dissociate in aqueous solution) in a 1.9 L solution= 0 M

[Cl-] in 0.65 g of LiCl (100 % dissociation) in a 1.9 L solution= {(0.65g /42.394g/mol)/1.9 L} = 0.008 M

[Cl-] in 0.65 g of NiCl2(100% dissociation with 1 mole of NiCl2 giving 2 moles of Cl-) in a 1.9 L solution

= 2*{(0.65g /129.59 g/mol)/1.9 L} = 0.0053 M

[Cl-] in 0.65 g of Ba(ClO2)2 in a 1.9 L solution= 0 M since Ba(ClO2)2 will dissociate to give Ba2+ and 2ClO2-, but no Cl-.