# Problem: Your lab partner messes up and accidentally makes the needed solution of NaCl too concentrated, 150.0 mL of a 0.78 M solution, when you needed 150.0 mL of a 0.45 M solution. You sigh, and add water to dilute the solution. What is the final volume of your corrected 0.45 M NaCl solution?A. 86.5 mLB. 1,730 mLC. 260. mLD. 520. mL E. 192 mL

###### FREE Expert Solution

We are being asked to find the volume of 0.45 M NaCl can be prepared by diluting 150 mL of 0.78 M NaCl.

When we are adding water (or solvent) to a solution to decrease its concentration, we are diluting the solution. When dealing with dilution we will use the following equation:

$\overline{){{\mathbf{M}}}_{{\mathbf{1}}}{{\mathbf{V}}}_{{\mathbf{1}}}{\mathbf{=}}{{\mathbf{M}}}_{{\mathbf{2}}}{{\mathbf{V}}}_{{\mathbf{2}}}}$

M1 = initial concentration
V1 = initial volume
M2 = final concentration
V2 = final volume

Calculate the final volume of the 0.45 M NaCl solution.

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###### Problem Details

Your lab partner messes up and accidentally makes the needed solution of NaCl too concentrated, 150.0 mL of a 0.78 M solution, when you needed 150.0 mL of a 0.45 M solution. You sigh, and add water to dilute the solution. What is the final volume of your corrected 0.45 M NaCl solution?

A. 86.5 mL

B. 1,730 mL

C. 260. mL

D. 520. mL

E. 192 mL