To what final volume should you dilute 50.5ml of a 4.75 M KI solution so that 27.5ml of the diluted solution contains 3.10g of KI

Never mind i figured it out:)

You have a 10 M acidic solution. However, you need that solution to be 0.25 M. How many ml of 10 M should be diluted to obtain 300 ml of 0.25 M acid solution?

To find the final volume to which you should dilute the solution, you can use the equation:

M1V1 = M2V2

where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.

First, let's calculate the initial moles of KI in the initial solution:

Moles = Molarity × Volume
Moles = 4.75 M × 50.5 ml
Moles = 239.875 mmol

Next, let's calculate the moles of KI in the 27.5 ml of the diluted solution:

Moles = Mass / Molar Mass
Moles = 3.10 g / 166.0028 g/mol
Moles = 0.018674 mol

Now, we can use the equation to find the final volume:

M1V1 = M2V2
(4.75 M) × (50.5 ml) = (0.018674 mol) × V2

V2 = (4.75 M × 50.5 ml) / (0.018674 mol)
V2 ≈ 12804.5 ml

Therefore, you should dilute the initial 50.5 ml solution to a final volume of approximately 12804.5 ml.