1. You dissolve 157.1 g of ammonium nitrate in a 250 mL volumetric flask and add water to the mark (call this solution A). You take 30 mL of solution A and place it in a 100 mL volumetric flask and add water to the mark (this is solution B). Next you take 50 mL of solution B and place it in a 500 mL volumetric flask and add water to the mark (this is solution C). Finally you take 10 mL of solution A, 10 mL of solution B and 10 mL of solution C and mix them to form solution D. What is the concentration (M) of solution D? (see problem 6 in Zumdahl test bank)
To find the concentration (M) of solution D, we need to understand the concept of dilution and use the information given.
Let's break down the process step by step:
Solution A:
- Dissolved 157.1 g of ammonium nitrate in a 250 mL volumetric flask and added water to the mark.
Solution B:
- Took 30 mL of Solution A and placed it in a 100 mL volumetric flask and added water to the mark.
Solution C:
- Took 50 mL of Solution B and placed it in a 500 mL volumetric flask and added water to the mark.
Solution D:
- Mixed 10 mL of Solution A, 10 mL of Solution B, and 10 mL of Solution C.
To find the concentration (M) of Solution D, we need to know the concentration of the original solution, Solution A. However, the problem does not provide the molarity or volume of Solution A, so we cannot directly calculate the concentration of Solution D using the given information.
If we are given the molarity of Solution A, we can calculate the concentration of Solution D using the following formula:
M1V1 = M2V2
Where:
M1 = initial molarity (concentration) of the solution
V1 = initial volume of the solution
M2 = final molarity (concentration) of the solution
V2 = final volume of the solution
Without the molarity of Solution A, we cannot determine the concentration of Solution D.