I am having trouble getting this starting and figuring out the correct steps...the problem is
Calculate the final concentration of the solution in each question
1) Water is added to 0.270 L of a 6.00M HCl solution to give a volume of 3.00 L (Express answers with the appropriate units)?
2) A 31.0 mL sample of a 2.50 M KCl solution is diluted with water to 0.350L (Express answers with the appropriate units)?
I think the answer for #2 may be 0.221 M? Is this correct?
mL x M = mL x M or
L x M = L x M
There aren't many dilution problems this one can't do.
I just figured out the first one shortly after I answered the second question thank you
To calculate the final concentration of a solution, you need to use the formula:
C1V1 = C2V2
Where:
C1 = initial concentration
V1 = initial volume
C2 = final concentration
V2 = final volume
Let's go through each question step by step to find the final concentration.
1) Water is added to 0.270 L of a 6.00 M HCl solution to give a volume of 3.00 L.
In this case, the initial concentration of HCl (C1) is given as 6.00 M, and the initial volume (V1) is 0.270 L. The final volume (V2) after adding water is 3.00 L. We need to find the final concentration (C2).
Using the formula C1V1 = C2V2, we can plug in the values:
(6.00 M)(0.270 L) = C2(3.00 L)
Now, let's solve for C2:
C2 = (6.00 M)(0.270 L) / (3.00 L)
C2 = 0.54 M
So, the final concentration of the HCl solution is 0.54 M.
2) A 31.0 mL sample of a 2.50 M KCl solution is diluted with water to 0.350 L.
Here, the initial concentration (C1) of KCl is 2.50 M, the initial volume (V1) is 31.0 mL (which needs to be converted to liters), and the final volume (V2) is 0.350 L. We need to find the final concentration (C2).
First, we convert the initial volume from mL to L:
V1 = 31.0 mL / 1000 mL/L
V1 = 0.031 L
Using the formula C1V1 = C2V2, we can substitute the values:
(2.50 M)(0.031 L) = C2(0.350 L)
Solving for C2:
C2 = (2.50 M)(0.031 L) / (0.350 L)
C2 = 0.223 M
So, the final concentration of the KCl solution is 0.223 M.