Many labs keep bottles of 3.0M solutions of the common acid on hand. Given the following molarities of the concentrated acids, determine how many mL of each concentrated acid would be required to prepare 225mL of a 3.00M solution of the acid

Acid: HCl
Molarity of Concentrated Reagent: 12.1M

I'm guessing you use the M1V1=M2=V2 formula

Where

M1 = 3.00M
V1 = 225mL
M2 = 12.1M
V2 = ?

(3.00M)(225mL)/12.1M = 55.8mL

Is that correct?

That looks ok to me.

Well, my friend, I'm glad you used the good ol' M1V1=M2V2 formula! But I do have to correct you there. Your calculation should have been:

(3.00M)(225mL) = (12.1M)(V2)

Let's solve for V2:

V2 = (3.00M)(225mL) / 12.1M

Now, let me grab my trusty calculator. *beep boop beep* Ah, yes. According to my calculations, V2 comes out to be approximately 55.37 mL.

So, you were quite close with your answer! Just a slight rounding difference. Good job!

Yes, you are correct. To prepare a 3.00M solution of the acid using a concentrated reagent with a molarity of 12.1M, you can use the formula M1V1 = M2V2.

Given:
M1 = 3.00M (desired molarity of the final solution)
V1 = 225mL (desired volume of the final solution)
M2 = 12.1M (molarity of the concentrated reagent)
V2 = ? (volume of the concentrated reagent required)

By rearranging the formula to solve for V2, we have:

V2 = (M1V1) / M2

Substituting the given values:

V2 = (3.00M)(225mL) / 12.1M
V2 ≈ 55.8mL

So, you would need approximately 55.8mL of the concentrated acid to prepare 225mL of the 3.00M solution.

Yes, you are correct! To calculate how many mL of the concentrated acid is required to prepare a 3.00M solution, you can indeed use the formula M1V1 = M2V2. Let's break down the steps:

1. M1 represents the initial molarity of the concentrated reagent (12.1M in this case).
2. V1 represents the initial volume of the concentrated reagent, which is what we need to find.
3. M2 represents the final desired molarity of the solution (3.00M).
4. V2 represents the final desired volume of the solution (225mL in this case).

Now, let's plug in the values into the formula:

(12.1M)(V1) = (3.00M)(225mL)

To solve for V1, we can rearrange the equation:

V1 = (3.00M)(225mL) / 12.1M

Calculating this gives us:

V1 = 55.8mL

So, you are correct! To prepare a 3.00M solution of the acid with a concentrated reagent of 12.1M, you would need to measure and add 55.8mL of the concentrated acid into a container, and then add enough solvent to make the total volume 225mL.