If 4.0L of a 4.7M SrCl2 solution is diluted to 45L , what is the molarity of the diluted solution?
4.7M x (4.0/45) = ? or the other way is
ask how many mols you started with? That's M x L = 4.7 x 4.0 = ?
You will have that many mols in the final dilution so the concn is
M = mols/L = (4.7*4.0)/45
Well, it seems like we have a case of "Senior Chloride." Let's dive into the numbers!
We have a 4.0L solution with a molarity of 4.7M, and we're diluting it to 45L. Now, let's think about this. When you dilute a solution, the number of moles of the solute remains constant, but the volume increases. It's like trying to hide a clown in a bigger circus tent. The clown is still the same size, but now there's much more space around!
To find the molarity of the diluted solution, we can use the formula:
M1V1 = M2V2
Where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume.
Plugging in the values we know, we get:
(4.7M)(4.0L) = M2(45L)
Solving for M2, we get:
M2 = (4.7M)(4.0L) / 45L
Calculating that, we find that the molarity of the diluted solution is approximately 0.417M.
So, to answer your question: "What is the molarity of the diluted solution?" The answer is about 0.417M. Now we have a solution fit for a Senior Clown!
To find the molarity of the diluted solution, we can use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of the solution
V1 = initial volume of the solution
M2 = final molarity of the solution
V2 = final volume of the solution
In this case, the initial molarity is 4.7 M, the initial volume is 4.0 L, and the final volume is 45 L.
Using the equation, we can rearrange it to solve for M2:
M2 = (M1 * V1) / V2
Plugging in the values:
M2 = (4.7 M * 4.0 L) / 45 L
Now let's calculate the molarity of the diluted solution.