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To what volume should you dilute 131ml of an 7.95M CuCl2 solution so that 50.5ml of the diluted solution contains 5.8g CuCl2?
Wiki User
∙ 14y ago
First multiply .131ml and 7.95M to get the moles of Cucl2. (You will need this later)
Then find the moles per 49.5ml diluted solution. (6.1g divided my molar mass)
Then set both equal to each other
Original mol/X = Diluted mol/49.5ml and solve for X
This should work
Wiki User
∙ 12y ago
Wiki User
∙ 14y agoThis is just a matter of changing the density. You want to get 5.8g/50.5mL. You currently have 7.95 moles/Liter of CuCl2. 1 mole of CuCl2 is roughly 134.5g. Therefore 7.95 moles/Liter of CuCl2 is roughly 1069.275g/L=1.069g/mL.=1g/0.9352mL
5.8g/50.5mL= 1g/8.707mL. So you need to add some amount to .9352mL to get to 8.707mL. Well this is now simply subtraction. 8.707-.9352=7.7718
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