🤓 Based on our data, we think this question is relevant for Professor King's class at DREXEL.

We’re being asked to calculate the concentration of sodium ions (Na^{+}) in ppm in the sample solution.

Let’s first define **ppm** and **ppb**.

• **1 ppm means 1 part of solute for every 10 ^{6} parts of the solution**

*Can be written as:*

$\overline{){\mathbf{ppm}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solute}}{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}{\mathbf{\times}}{{\mathbf{10}}}^{{\mathbf{6}}}}$

• **1 ppb means 1 part of solute for every 10 ^{9} parts of the solution**

A 4.55 L sample of solution contains 0.115 g of sodium ions. Determine the concentration of sodium ions in ppm if the density of the solution is 1.00 g/mL.

A. 52.3 ppm

B. 13.2 ppm

C. 12.7 ppm

D. 25.3 ppm

E. 36.5 ppm