In order to dilute 1L of 6M solution of NaOH to .5M solution, how much water must be added?
mL x M = mL x M
1000 mL x 6M = mL x 0.5M
Solve for mL which gives th TOTAL volume needed.
its actually the other way around, u need to figure out what volume u need of the .5M, e.g., if u want to make 500ml of it then u wud use c1vi=c2v2
so .5L X .5M = xL X 6M
making xL subject of the formula u wud then have the volume of ^M NaOH u wud need to put in 500ml to get a .5M solution
To dilute a 1L solution of 6M NaOH to a 0.5M solution, we can use the formula for dilution:
C1V1 = C2V2
Where:
C1 = Initial concentration (6M)
V1 = Initial volume (1L)
C2 = Final concentration (0.5M)
V2 = Final volume (unknown)
Rearranging the formula, we get:
V2 = (C1V1) / C2
Substituting the values:
V2 = (6M x 1L) / 0.5M
V2 = 12L
Therefore, to dilute the solution to 0.5M, you need to add 12L of water.
To dilute a solution, you need to add a certain volume of solvent (in this case, water) to the original solution. The amount of water needed can be calculated using the formula:
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 want to dilute a 6M solution of NaOH to 0.5M. Let's assume V1 is the volume of the 6M solution that needs to be diluted.
C1 = 6M
V1 = ?
C2 = 0.5M
V2 = 1L (since we want the final volume to be 1L)
Rearranging the formula, we get:
V1 = (C2 x V2) / C1
Substituting the values, we have:
V1 = (0.5M x 1L) / 6M
V1 = 0.0833 L
Therefore, you need to add approximately 0.0833 liters (or 83.3 ml) of water to dilute 1 liter of a 6M solution of NaOH to a 0.5M solution.