Question

A crazy person breaks into the school and starts randomly mixing chemical solutions together.

They combine a 0.7 M solution with a volume of 800 mL, a 1 M solution with a volume of 300 mL, and a 1.9 M solution with a volume of 860 mL into a large container. Assuming the final product doesn't blow up, what will the final solution's molarity be?

Answer 1

To calculate the final molarity of the solution, we will need to use the principle of conservation of moles.

First, we need to calculate the number of moles of each solute in the solution. We can use the formula:

moles = concentration (in moles/L) x volume (in L)

For the 0.7 M solution:
moles = 0.7 mol/L x 0.8 L = 0.56 moles

For the 1 M solution:
moles = 1 mol/L x 0.3 L = 0.3 moles

For the 1.9 M solution:
moles = 1.9 mol/L x 0.86 L = 1.634 moles

Next, we need to add up the total number of moles of solute in the solution:

total moles = 0.56 moles + 0.3 moles + 1.634 moles = 2.494 moles

Finally, we need to calculate the molarity of the final solution using the formula:

molarity = total moles / total volume (in L)

The total volume of the solution is:

total volume = 0.8 L + 0.3 L + 0.86 L = 1.96 L

Therefore, the molarity of the final solution is:

molarity = 2.494 moles / 1.96 L = 1.27 M

So the final solution's molarity is 1.27 M, assuming that no reaction occurs between the chemicals.