Question

A 4.55 l sample of water 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.

Answer 1

When one talks about ppm in a liquid solution someone means mg/L so we would not be using the density. This usually means ug/g or mg/kg 0.115 g Na^+ * 10^6 ug/1 g = 115000 ug/g 4.55 L * 1000 mL/1L = 4550 mL Concentration of Na^+ in ppm: 115000 ug/g /4550 mL = 25.27 pm of sodium ion

Answer 2

Answer: 25.3 ppm

Explanation: ppm stands for parts per million. It's a way for representing concentrations when a very small amount of solute is dissolved in the solvent.

1ppm = $\frac{1mg}{L}$

From given information, 0.115 grams of sodium ions(solute) dissolved in 4.55 L sample of water.

Let's convert the grams of solute to mg.

1 g = 1000 mg

$0.115g(\frac{1000mg}{1g})$

= 115 mg

Let's divide the mg of solute by liters of solution to get the ppm concentration.

$\frac{115mg}{4.55L}$

= 25.3 ppm

(Note- mass of solute is very much negligible as compared to the mass of solution, so mass of solute is almost same as the mass of solution)

So, the concentration of sodium ions in ppm will be 25.3 .