Given 1.2 L of a 2.2 M sodium sulfate solution, calculate the volume in liters you would need to

Given 1.2 L of a 2.2 M sodium sulfate solution, calculate the volume in liters you would need to add to obtain a 0.5 M solution of sodium sulfate??

How to I go about solving this problem? is there a formula I can use?? Can you guide me through please?? Thanksss so much

We will use C1V1=C2V2. This simply states that the initial volume times the initial concentration is equal to the final volume time the final concentration.

Plug and chug.

(2.2M)(1.2L)=(0.5M)(V2)
V2=5.28L
So we need to add 5.3L to get a 0.5M solution of sodium sulfate.

You need to find the number of moles (n) of Na2SO4.
You manipulate the molarity formula (M = n/V) to solve for moles (n). Where M is the molarity and n represents the moles. V = the volume in liters.

n = M(V) = 2.2(1.2) = 2.64 moles of Na2SO4.

You then manipulate the molarity formula to solve for V with your known molarity (.5) and moles (2.64) to get the volume needed.

V = n/M = 2.64/.5 = 5.3 L -- I believe that is correct.