Question

Find the solution to a chemistry problem where 50.0 mL of 1.20 M NaOH is diluted to 250 mL and determine the resulting concentration

Answer 1

To find the resulting concentration after diluting a solution, you can use the dilution formula:

\[
C_1 V_1 = C_2 V_2
\]

Where:
- \(C_1\) is the initial concentration,
- \(V_1\) is the initial volume,
- \(C_2\) is the final concentration,
- \(V_2\) is the final volume.

In this problem:
- \(C_1 = 1.20 \, \text{M}\)
- \(V_1 = 50.0 \, \text{mL}\)
- \(V_2 = 250 \, \text{mL}\)

Now, we need to find \(C_2\). Rearranging the equation gives:

\[
C_2 = \frac{C_1 V_1}{V_2}
\]

Now substituting the values:

\[
C_2 = \frac{(1.20 \, \text{M})(50.0 \, \text{mL})}{250 \, \text{mL}}
\]

Calculating the numerator:

\[
1.20 \, \text{M} \times 50.0 \, \text{mL} = 60.0 \, \text{mol·mL/M} = 60.0 \, \text{mol}
\]

Now, substituting this into the equation:

\[
C_2 = \frac{60.0 \, \text{mol}}{250 \, \text{mL}} = 0.240 \, \text{M}
\]

Thus, the resulting concentration after dilution is:

\[
C_2 = 0.240 \, \text{M}
\]