How many ml of .050 M NaOH are required to prepare 1500.0 mL of .0020 M NaOH? Please show work, I'm not sure how to do this. Thanks!
answered above.
you are diluting it a factor of
.05/.002= 25 times
24 parts water, 1 part orig solution.
each part will be equal to 1500/25=60ml
The "text" way to solve this is to find the moles of NaOH in the final solution
moles=volume*M=1.500*.002=.003 moles
then find the volume in the original solution with that many moles..
volume=.003/.05=60 ml Same result
To solve this problem, you can use the formula:
Moles = Molarity x Volume
First, let's determine the number of moles of NaOH needed to prepare the desired solution.
Moles of NaOH = Molarity x Volume
Moles of NaOH = 0.0020 mol/L x 1500.0 mL
Note that we need to convert the volume from mL to L to match the units of the molarity. Since there are 1000 mL in 1 L, we can convert the volume as follows:
Moles of NaOH = 0.0020 mol/L x (1500.0 mL / 1000 mL)
Now we can calculate the number of moles of NaOH needed:
Moles of NaOH = 0.0020 mol/L x 1.5000 mol
Next, let's determine the amount of 0.050 M NaOH required to obtain that number of moles.
Moles of NaOH = Molarity x Volume
Moles of NaOH = 0.050 mol/L x Volume
To find the volume, we rearrange the equation:
Volume = Moles of NaOH / Molarity
Volume = (0.0020 mol) / (0.050 mol/L)
Finally, we can calculate the volume of 0.050 M NaOH needed:
Volume = 0.040 L
Therefore, you will need 40 mL of 0.050 M NaOH to prepare 1500.0 mL of 0.0020 M NaOH solution.