A 230.-mL sample of a 0.280 M CaCl2 solution is left on a hot plate overnight; the following morning, the solution is 1.10 M. What volume of water evaporated from the 0.280 M CaCl2 solution?

230mL of .280M solution contains 0.0644 moles CaCl2

x L of 1.1M solution now contains the .0644 moles, so x = 0.0585 = 58.5 mL

so, subtract to find the difference, which evaporated.

Well, looks like we have a little H2O disappearing act here! Let's calculate the volume of water that decided to make a great escape.

We know that the initial concentration of the CaCl2 solution was 0.280 M, and after the evaporation, it turned into a 1.10 M solution. So the concentration increased by 1.10 - 0.280 = 0.820 M.

Now let's use the equation:

(initial concentration)(initial volume) = (final concentration)(final volume)

We can rearrange this equation to solve for the final volume of the solution:

final volume = (initial concentration)(initial volume) / final concentration

Plugging in the values we have:

final volume = (0.280 M)(230 mL) / 1.10 M

Calculating this, we find that the final volume of the solution is approximately 58.36 mL.

Now, we know that the volume of water evaporated is the initial volume minus the final volume:

volume of water evaporated = initial volume - final volume
= 230 mL - 58.36 mL
= 171.64 mL

So it seems like about 171.64 mL of water decided to pull a disappearing act and leave the party!

To find the volume of water evaporated from the 0.280 M CaCl2 solution, we need to calculate the initial moles of CaCl2 and final moles of CaCl2, and then use the difference to determine the moles of water evaporated.

First, let's calculate the initial moles of CaCl2 in the solution:
Initial moles of CaCl2 = initial concentration x initial volume
= 0.280 M x 230 mL
= 64.4 moles

Next, we need to calculate the final moles of CaCl2 in the solution:
Final moles of CaCl2 = final concentration x final volume
= 1.10 M x 230 mL
= 253 moles

The change in moles of CaCl2 is the difference between the final moles and initial moles:
Change in moles of CaCl2 = final moles - initial moles
= 253 moles - 64.4 moles
= 188.6 moles

Since CaCl2 is a salt and does not evaporate, the change in moles represents the moles of water evaporated. However, to find the volume, we need to convert moles to volume using the concentration of water (which is approximately 55.5 M):

Change in volume = Change in moles / concentration of water
= 188.6 moles / 55.5 M
≈ 3.39 mL

Therefore, approximately 3.39 mL of water evaporated from the 0.280 M CaCl2 solution.

To find the volume of water that evaporated from the 0.280 M CaCl2 solution, we can use the dilution equation:

C1V1 = C2V2

Where:
C1 = initial concentration
V1 = initial volume
C2 = final concentration
V2 = final volume

In this case, the initial concentration is 0.280 M, the initial volume is 230 mL, the final concentration is 1.10 M, and we need to find the final volume (V2).

Let's solve the equation for V2:

C1V1 = C2V2

0.280 M * 230 mL = 1.10 M * V2

64.4 = 1.10V2

V2 = 64.4 / 1.10

V2 ≈ 58.55 mL

Therefore, the volume of water that evaporated from the 0.280 M CaCl2 solution is approximately 58.55 mL.