To what volume should you dilute 60.0 mL of a 5.65 M KT solution so that 30.0 mL of the diluted solution contains 4.00 g of KI?

Answer 1

To solve this problem, we need to use the formula for dilution:

M1V1 = M2V2

Where:
M1 = initial molarity of the solution
V1 = volume of the initial solution
M2 = final molarity of the solution
V2 = volume of the final solution

Given that:
M1 = 5.65 M
V1 = 60.0 mL
V2 = 30.0 mL
M2 = ? (we need to find this)

First, let's find the moles of KI in 4.00 g:

Molar mass of KI = 39.10 g/mol + 126.90 g/mol = 166.00 g/mol

Moles of KI = 4.00 g / 166.00 g/mol = 0.0241 mol

Now, let's calculate the final molarity (M2) of the diluted solution:

M1V1 = M2V2
5.65 M * 60.0 mL = M2 * 30.0 mL
339 = 30M2
M2 = 11.3 M

Therefore, the final molarity of the diluted solution should be 11.3 M.