What is the molarity of the final solution of 2.00mL of the 5.00M stock solution is diluted to 10.00mL to make solution A. Solution A undergoes a second dilution by taking 3.00mL solution A and diluting it to 25mL?
I'm so confused by this. Please help.
Use mL1 x M1 = mL2 x M2 and it will work out OR, logic. Logic goes this way.
5.00M x (2.00/10.00) x (3.00/25.00) = ?
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Oh boy, it's dilution time! Don't worry, I'm here to clown around and help you out. Let's break it down step by step:
First, we need to find the molarity of solution A. We know that 2.00mL of the 5.00M stock solution is diluted to 10.00mL to make solution A. So to find the molarity of A, we'll use the formula:
(M1)(V1) = (M2)(V2)
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 get:
(5.00M)(2.00mL) = (M2)(10.00mL)
Solving for M2, we get:
M2 = (5.00M)(2.00mL) / (10.00mL)
M2 = 1.00M
So solution A has a molarity of 1.00M.
Now let's move on to the second dilution. We're taking 3.00mL of solution A and diluting it to 25mL. Using the same formula, we can find the molarity of the final solution.
(1.00M)(3.00mL) = (M3)(25mL)
Solving for M3, we get:
M3 = (1.00M)(3.00mL) / (25mL)
M3 = 0.12M
And there you have it, the molarity of the final solution after the second dilution is 0.12M. Ta-da!
Sure! I can help you understand this problem.
To find the molarity of the final solution, we need to go through two dilutions:
1. The first dilution:
We start with a 2.00 mL sample from a 5.00 M stock solution and dilute it to a total volume of 10.00 mL, resulting in solution A.
To calculate the new molarity, we can use the formula:
M1 x V1 = M2 x V2
M1 = molarity of the stock solution = 5.00 M (given)
V1 = volume of the stock solution used = 2.00 mL
M2 = molarity of the diluted solution (solution A) = ?
V2 = total volume of the diluted solution = 10.00 mL (given)
Plugging the known values into the formula:
5.00 M x 2.00 mL = M2 x 10.00 mL
Solving for M2:
M2 = (5.00 M x 2.00 mL) / 10.00 mL
= 10.00 M / 10.00
= 1.00 M
Therefore, the molarity of solution A after the first dilution is 1.00 M.
2. The second dilution:
Now, we take a 3.00 mL sample from solution A and dilute it to a total volume of 25 mL.
Again, we can use the formula:
M1 x V1 = M2 x V2
M1 = molarity of solution A = 1.00 M
V1 = volume of solution A used = 3.00 mL
M2 = molarity of the final solution = ?
V2 = total volume of the final solution = 25 mL (given)
Plugging the known values:
1.00 M x 3.00 mL = M2 x 25 mL
Solving for M2:
M2 = (1.00 M x 3.00 mL) / 25 mL
= 3.00 M / 25
= 0.12 M
So, the molarity of the final solution, after both dilutions, is 0.12 M.
I hope this explanation clarifies the process for you! Let me know if you have any further questions.