What is the molarity of the solution prepared by diluting 25.0ml of 0.220M NaCl to 75.0ml of final volume?( explain your steps)

There is no "explanation" as I see it.

mL x M = mL x M is the dilution formula or you can do it as
0.220M x (25/75) = ??
Also, you can say you have diluted it by a factor of 3 (25 to 75); therefore, it must be 1/3 of the original concn.

Well, let's dive in and find the molarity of the solution together!

Step 1: Calculate the number of moles of NaCl in the initial solution (25.0 ml of 0.220 M NaCl). We can use the formula:

moles = Molarity x Volume

moles = 0.220 M x (25.0 ml / 1000) L

moles = 0.220 M x 0.025 L

moles = 0.0055 mol

Step 2: Now that we know the number of moles of NaCl in the initial solution, we can use it to determine the molarity of the final solution. We'll use the same formula, but this time we'll solve for the molarity. Let's do the math:

Molarity = moles / Volume

Molarity = 0.0055 mol / (75.0 ml / 1000) L

Molarity = 0.0055 mol / 0.075 L

Molarity = 0.0733 M

So, the molarity of the final solution, prepared by diluting 25.0 ml of 0.220 M NaCl to 75.0 ml, is 0.0733 M. Voila!

To calculate the molarity of the solution prepared by dilution, use the formula:

M1V1 = M2V2

Where:
M1 = initial molarity
V1 = initial volume
M2 = final molarity
V2 = final volume

In this case:
M1 = 0.220 M (initial molarity of NaCl solution)
V1 = 25.0 mL (initial volume of NaCl solution)
V2 = 75.0 mL (final volume of diluted solution)
M2 = ?

Step 1: Convert the initial volume from milliliters (mL) to liters (L).
25.0 mL = 0.0250 L

Step 2: Plug the values into the formula:
(0.220 M) * (0.0250 L) = M2 * (0.0750 L)

Step 3: Solve for M2.
M2 = (0.220 M * 0.0250 L) / 0.0750 L

Step 4: Calculate M2.
M2 = (0.00550 mol) / 0.0750 L

Step 5: Convert the answer to the desired units.
M2 = 0.0733 M

Therefore, the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to a final volume of 75.0 mL is 0.0733 M.

To find the molarity of a solution prepared by dilution, 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.

In this case, we have:
M1 = 0.220 M (initial molarity)
V1 = 25.0 mL (initial volume)
M2 = ? (final molarity, what we want to find)
V2 = 75.0 mL (final volume)

We can plug the values into the formula and solve for M2:

(0.220 M)(25.0 mL) = M2(75.0 mL)

To solve for M2, we can rearrange the equation:

M2 = (0.220 M)(25.0 mL) / 75.0 mL

Now let's do the calculation:

M2 = (0.220 M)(25.0 mL) / 75.0 mL
= (5.50 mol/L * mL) / 75.0 mL
= 0.07333 M

Therefore, the molarity of the solution prepared by diluting 25.0 mL of 0.220 M NaCl to a final volume of 75.0 mL is 0.07333 M.