In order to prepare very dilute solutions, a lab technician chooses to perform a series of dilutions instead of measuring a very small mass. a solution was prepared by dissolving 0.360 g of kno3 in enough water to make 500. ml of solution. a 10.0 ml sample of this solution was transferred to a 500.0-ml volumetric flask and diluted to the mark with water. then 10.0 ml of the diluted solution was transferred to a 250.0-ml flask and diluted to the mark with water. what is the final concentration of the kno3 solution? 7.91 × 10-9 m1.42 × 10-4 m5.70 × 10-6 m2.85 × 10-6 m7.12 × 10-3 m

The final concentration of potassium nitrate is

Explanation:

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

We are given:

Mass of potassium nitrate (solute) = 0.360 g

Molar mass of potassium nitrate = 101.1 g/mol

Volume of solution = 500.0 mL

Putting values in above equation, we get:

To calculate the molarity of the diluted solution, we use the equation:

         .......(1)

are the molarity and volume of the concentrated solution

are the molarity and volume of diluted solution

We are given:

Putting values in equation 1, we get:

are the molarity and volume of the concentrated solution

are the molarity and volume of diluted solution

We are given:

Putting values in equation 1, we get:

Hence, the final concentration of potassium nitrate is

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