Question

You need to dilute 97mL of an 11M stock solution. What is the final molarity of the solution if you end up with 1, 157mL of solution after adding distilled water?

Answer 1

The final molarity of the solution after diluting 97mL of an 11M stock solution and adding distilled water to a final volume of 1,157mL is approximately 0.928M.

Step-by-step explanation:

To find the final molarity of the solution after dilution, we can use the equation:

M1V1 = M2V2

Where M1 and V1 are the initial concentration and volume of the stock solution, and M2 and V2 are the final concentration and volume of the solution after dilution.

In this case, the initial concentration of the stock solution is 11M, and the initial volume is 97mL. The final volume after adding distilled water is 1,157mL. Plugging in these values, we can calculate the final molarity:

(11M)(97mL) = (M2)(1,157mL)

Solving for M2, we get:

M2 = (11M)(97mL) / (1,157mL) = 0.928M