Question

What is the new molarity if you dilute a 1000.0 ml of a 3.0 M solution by doubling the volume?

Answer 1

To find the new molarity after diluting a solution, you can use the dilution formula:

\[
M_1 V_1 = M_2 V_2
\]

Where:
- \(M_1\) = initial molarity (3.0 M)
- \(V_1\) = initial volume (1000.0 mL)
- \(M_2\) = final molarity (unknown)
- \(V_2\) = final volume (double the initial volume, so 2000.0 mL)

First, you can plug in the known values into the equation:

\[
(3.0 \, \text{M}) \times (1000.0 \, \text{mL}) = M_2 \times (2000.0 \, \text{mL})
\]

Calculating the left side:

\[
3000 \, \text{M} \cdot \text{mL} = M_2 \times 2000.0 \, \text{mL}
\]

Now, solve for \(M_2\):

\[
M_2 = \frac{3000 \, \text{M} \cdot \text{mL}}{2000.0 \, \text{mL}} = 1.5 \, \text{M}
\]

So, the new molarity after diluting the solution is **1.5 M**.