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A 22.2 g sample of MgCl2 is dissolved in water, creating a solution with a mole fraction of 0.0500 moles of MgCl2 per mole of solution. The molar mass of MgCl2 is 95.21 g/mol. How many total moles of solution were created?

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This problem is providing both the mole fraction and mass of magnesium chloride in an aqueous solution. Thus, the total moles of the solution are required and turned out to be 4.62 moles.

Mole fraction

In chemistry, units of concentration are used to account for the relative amounts of solute and solvent in solid, liquid or even gaseous solutions.

Thus, several units are widely employed, yet this problem is about mole fraction, which relates the moles of the solute and the total moles of the solution as follows:

[tex]x=\frac{n_{solute}}{n_{total}}[/tex]

Hence, given the mass of the solute, calcium chloride, we can calculate its moles as follows:

[tex]n_{solute}=22.2g*\frac{1mol}{95.21g}=0.231mol[/tex]

Thereafter, we solve for the total moles of the solution and subsequently plug in the knowns:

[tex]n_{total}=\frac{n_{solute}}{x}\\\\n_{total}=\frac{0.231mol}{0.0500}\\\\n_{total}=4.62mol[/tex]

Learn more about mole fraction: https://brainly.com/question/2060778

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