Answer:
172 ml
Step-by-step explanation:
To determine the volume to which you should dilute 133 ml of a 7.95 M CuCl2 solution so that 52.0 mL of the diluted solution contains 4.20 g of CuCl2, you need to use the equation for molarity:
M = moles of solute / liters of solution
We know the moles of solute, which can be calculated from the mass of CuCl2 using the molar mass:
4.20 g CuCl2 / (1 mole CuCl2 / 134.45 g CuCl2) = 0.0311 moles CuCl2
And we know the volume of the diluted solution, which is 52.0 mL or 0.052 L. Plugging in these values, we can solve for the molarity of the diluted solution:
M = 0.0311 moles CuCl2 / 0.052 L = 0.596 M
Now that we know the molarity of the diluted solution, we can use the equation for dilution to determine the volume to which we should dilute the original solution:
C1V1 = C2V2
Where C1 and V1 are the concentration and volume of the original solution and C2 and V2 are the concentration and volume of the diluted solution. Plugging in the values, we have:
7.95 M * V1 = 0.596 M * 0.133 L
Solving for V1, we get:
V1 = 0.133 L * 0.596 M / 7.95 M = 0.0172 L = 172 mL
So, to achieve the desired concentration in 52.0 mL of the diluted solution, you should dilute 133 mL of the 7.95 M CuCl2 solution to a volume of 172 mL