What is the final concentration (M) of a solution prepared by diluting 50.0 mL of a 6.00 M KCl solution to a volume of 0.500 L?


A. 1.67
B. 0.600
C. 0.0167
D. 3.0
E. none of these

My initial thought was to take the 6.00 M KCl/0.500 L, for an answer of 12. This baffles me that the only answer suitable would be E. None of the above--I think I did something wrong.

Word of advice!!! Never take a Chemistry class online!!!

You are diluting 6.00 M solution from 50 to 500 mL; therefore, the final concn is

6.00 x (50/500) = 0.600 M

There is another, more fundamental way of doing this.
1. How many moles do you have in the 6.00 M solution. moles = M x L = 6.00 x 0.05 L = 0.300 moles.

2. How many moles do you have in the diluted solution? Of course, 0.300 moles.

3. What is the concn? The definition, remember, is M = moles/L; therefore, M = 0.300 moles/0.5 L = 0.600 M.

its 0.600

Ah, chemistry can be a tough nut to crack sometimes, can't it? Don't worry, I'm here to add a little humor and help you out!

So, let's solve this together. We can use the formula for dilution:

C1V1 = C2V2

Where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.

In this case, we have C1 = 6.00 M, V1 = 50.0 mL (which we'll need to convert to liters), and V2 = 0.500 L. We want to find C2, the final concentration.

First, let's convert V1 from milliliters to liters:

V1 = 50.0 mL = 50.0 mL * (1 L / 1000 mL) = 0.050 L

Now we can plug in the values and solve for C2:

6.00 M * 0.050 L = C2 * 0.500 L

0.300 M = C2 * 0.500 L

C2 = 0.300 M / 0.500 L

C2 = 0.600 M

So the final concentration is 0.600 M.

Therefore, the answer is B. 0.600.

Cheer up, chemistry isn't so bad! And don't be so hard on yourself for taking a class online. Just remember, even if chemistry gets a bit confusing, you've got humor on your side!

To find the final concentration of the solution after dilution, you can use the equation:

C1V1 = C2V2

Where:
C1 = initial concentration of the solution (in M)
V1 = initial volume of the solution (in L)
C2 = final concentration of the solution (in M)
V2 = final volume of the solution (in L)

Let's plug in the values given:

C1 = 6.00 M
V1 = 0.0500 L
V2 = 0.500 L (final volume after dilution)

Now, rearrange the equation to solve for C2:

C2 = (C1 * V1) / V2

C2 = (6.00 M * 0.0500 L) / 0.500 L

C2 = 0.600 M

So, the final concentration (M) of the solution after dilution is 0.600 M. Therefore, option B is the correct answer.

To find the final concentration (M) of the solution, you can use the dilution formula:

M1V1 = M2V2

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

In this case, the initial concentration (M1) is 6.00 M, the initial volume (V1) is 50.0 mL (which needs to be converted to liters by dividing by 1000), the final volume (V2) is 0.500 L, and we need to solve for the final concentration (M2).

Let's plug in the values into the dilution formula:

(6.00 M)(50.0 mL/1000) = M2(0.500 L)

First, convert 50.0 mL to liters by dividing by 1000: 50.0 mL / 1000 = 0.050 L

Now, rearrange the equation to solve for M2:

(6.00 M)(0.050 L) = M2(0.500 L)

Multiply 6.00 M by 0.050 L: 0.300 = M2(0.500 L)

Divide both sides of the equation by 0.500 L to isolate M2:

0.300 / 0.500 = M2

0.6 = M2

Therefore, the final concentration (M2) of the solution is 0.6 M.

So, the correct answer is B. 0.600.