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Chapter 4: Problem 104

A 230 -mL sample of a \(0.275-M \mathrm{CaCl}_{2}\) solution is left on a hot plate overnight; the following morning, the solution is 1.10\(M .\) What volume of water evaporated from the 0.275\(M \mathrm{CaCl}_{2}\) solution?

Short Answer

Expert verified
172.5 mL of water evaporated from the 0.275 M CaCl₂ solution.

Step by step solution

01

Calculate the initial moles of CaCl₂

First, we need to find the initial moles of CaCl₂ using the initial concentration and volume of the solution. The formula for calculating moles is: Moles = Concentration × Volume Here, the initial concentration of CaCl₂ is 0.275 M, and the initial volume is 230 mL. We will convert the volume to liters: 230 mL × (1 L / 1000 mL) = 0.230 L Now, we can calculate the initial moles of CaCl₂: Moles of CaCl₂ = 0.275 M × 0.230 L = 0.06325 mol
02

Calculate the final moles of CaCl₂

Since the moles of CaCl₂ remain constant after the evaporation of water, the final moles of CaCl₂ are the same as the initial moles: Final moles of CaCl₂ = 0.06325 mol
03

Calculate the final volume of the solution

Next, we will find the final volume of the CaCl₂ solution using the final concentration and the final moles of CaCl₂. The formula to calculate the volume is: Volume = Moles / Concentration The final concentration of CaCl₂ is given as 1.10 M. We can now calculate the final volume of the solution: Final volume = 0.06325 mol / 1.10 M = 0.0575 L
04

Calculate the volume of water that evaporated

Now, we can calculate the volume of water that evaporated from the initial solution by comparing the initial and final volumes of the solution: Initial volume - Final volume = Volume of water evaporated 0.230 L - 0.0575 L = 0.1725 L
05

Convert the volume to milliliters

Finally, we will convert the volume of evaporated water to milliliters: 0.1725 L × (1000 mL / 1 L) = 172.5 mL So, 172.5 mL of water evaporated from the 0.275 M CaCl₂ solution.

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