Question

A chemist must dilute 12.6mL of 7.27 M aqueous sodium nitrate (NaNO3) solution until the concentration falls to 6.00 M.He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

Answer 1

Answer:

The final volume is 15.3 mL

Explanation:

According to law of equivalence-

                                   $C_{1}V_{1}=C_{2}V_{2}$

where $C_{1}$ is initial concentration, $C_{2}$ is the final concentration, $V_{1}$ is the initial volume and $V_{2}$ is the final volume.

Here $C_{1}$ = 7.27 M, $V_{1}$ = 12.6 mL, $C_{2}$ = 6.00 M

So, $V_{2}=\frac{C_{1}V_{1}}{C_{2}}=\frac{7.27\times 12.6}{6.00}mL=15.3 mL$

So the final volume is 15.3 mL