Questions: In the laboratory, a student dilutes 13.3 mL of a 11.8 M hydrobromic acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution? Concentration = M

Determine the concentration of the diluted solution.

Identify the initial conditions.

The initial volume of the hydrobromic acid solution is \(13.3 \, \text{mL}\) and its concentration is \(11.8 \, \text{M}\).

Identify the final conditions.

The final volume of the solution after dilution is \(150.0 \, \text{mL}\).

Use the dilution formula.

The dilution formula is given by:

\[ C_1V_1 = C_2V_2 \]

where \(C_1\) is the initial concentration, \(V_1\) is the initial volume, \(C_2\) is the final concentration, and \(V_2\) is the final volume.

Substitute the known values into the dilution formula.

Substitute \(C_1 = 11.8 \, \text{M}\), \(V_1 = 13.3 \, \text{mL}\), and \(V_2 = 150.0 \, \text{mL}\) into the formula:

\[ 11.8 \, \text{M} \times 13.3 \, \text{mL} = C_2 \times 150.0 \, \text{mL} \]

Solve for the final concentration \(C_2\).

Rearrange the equation to solve for \(C_2\):

\[ C_2 = \frac{11.8 \, \text{M} \times 13.3 \, \text{mL}}{150.0 \, \text{mL}} \]

Calculate:

\[ C_2 = \frac{156.94 \, \text{M} \cdot \text{mL}}{150.0 \, \text{mL}} = 1.046 \, \text{M} \]

\(\boxed{1.046 \, \text{M}}\)

The concentration of the diluted solution is \(\boxed{1.046 \, \text{M}}\).