If 150.0 mL of 1.00 M C6H12O6 are diluted to 750.0 mL, what is the molarity of the final solution?
____ M?
mL1 x M1 = mL2 x M2
Use Dilution Equation (M1V1 = M2V2) to solve this problem.
M1=1.00mols/L
M2=?
V1=150.0mL, convert to Liter
V1=150mL*(1L/1000mL)=.15L
Do the same to V2
V2=750.0mL(1L/1000mL)=.75L
plug in the numbers into the Equation
M1V1=M2V2
M2=M1V1/V2, M2=(1mols/L)*(.15L)/(.75L)=.2M
The molarity of the final Solution is .2M.
To find the molarity of the final solution, 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, the initial volume (V1) is given as 150.0 mL, the initial molarity (M1) is given as 1.00 M, and the final volume (V2) is given as 750.0 mL.
Substituting the values into the formula, we have:
1.00 M * 150.0 mL = M2 * 750.0 mL
Now, we can solve for M2, the molarity of the final solution:
M2 = (1.00 M * 150.0 mL) / 750.0 mL
M2 = 0.20 M
Therefore, the molarity of the final solution is 0.20 M.