Question

The student then takes a 1.00M stock solution of table sugar (sucrose C12H22O11) and mixes 0.305L of stock solution with additional distilled water to create a dilute solution with a total volume of 1.25L.

Explain how the student can determine the molarity of the resulting solution. Show a valid calculation for the final molarity. PLS HELP

Answer 1

Answer: The molarity of final solution is 0.244 M.

Step-by-step explanation:

Given:
`M_(1)` = 1.00 M,
`V_(1)` = 0.305 L

`M_(2)` = ?,
`V_(2)` = 1.25 L

Formula used to calculate the molarity f resulting solution is as follows.

`M_(1)V_(1) = M_(2)V_(2)`

Substitute the values into above formula as follows.

`M_(1)V_(1) = M_(2)V_(2)\\1.00 M * 0.305 L = M_(2) * 1.25 L\\M_(2) = (1.00 M * 0.305 L)/(1.25 L)\\= 0.244 M`

Thus, we can conclude that the molarity of final solution is 0.244 M.