if I add water to 100.0 mL of a 0.15 M NaOH solution until the final volume is 150.0 mL what will the molarity of the diluted solution be? If I set this up properly I believe it is 0.10 M.....am I correct?
0.1M is correct.
0.15M x (100 mL/150 mL) = ?
To determine the molarity of the diluted solution, you can use the formula:
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, we have:
M1 = 0.15 M
V1 = 100.0 mL
V2 = 150.0 mL
Now, rearrange the formula to solve for M2:
M2 = (M1 * V1) / V2
Substitute the given values into the equation:
M2 = (0.15 M * 100.0 mL) / 150.0 mL
M2 = 0.10 M
So, you are correct. The molarity of the diluted solution is indeed 0.10 M.
To determine the molarity of the diluted solution, you can use the dilution formula:
C1V1 = C2V2
Where:
C1 = initial molarity of the solution (0.15 M)
V1 = initial volume of the solution (100.0 mL)
C2 = final molarity of the solution (what we want to find)
V2 = final volume of the solution (150.0 mL)
Now, let's solve for C2:
(0.15 M)(100.0 mL) = C2(150.0 mL)
Divide both sides by 150.0 mL:
(0.15 M)(100.0 mL) / 150.0 mL = C2
Calculating:
0.10 M = C2
Therefore, you are correct. The molarity of the diluted solution will be 0.10 M.