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aleksandr82 [10.1K]
3 years ago
12

What is the molariity of a 50.0 mL aqueous solution containing 10.0 grams of copper (II) sulfate, CuSO4?

Chemistry
1 answer:
jolli1 [7]3 years ago
3 0

Answer:

The molarity is 1.26 \frac{ moles}{L}

Explanation:

Molarity is a unit of concentration that is based on the volume of a solution and represents the number of moles of solutes contained in a liter. The molarity of a solution is calculated by dividing the moles of the solute by the liters of the solution and is expressed in units (moles / liter).

Molarity=\frac{number of moles of solute}{Volume}

You must calculate the number of moles of CuSO₄. So, being:

  • Cu: 63.54 g/mole
  • S: 32 g/mole
  • O: 16 g/mole

the molar mass of CuSO₄ is

CuSO₄=63.54 g/mole + 32 g/mole + 4* 16 g/mole= 159.54 g/mole

Then it is possible to apply the following rule of three: if 159.54 g of CuSO₄ are present in 1 mole, 10 g in how many moles are they?

moles=\frac{10 g*1 mole}{159.54 g}

moles= 0.063 moles

Then:

  • number of moles of solute= 0.063 moles
  • Volume= 50 mL= 0.05 L (Being 1L=1000 mL)

Replacing in the definition of molarity:

Molarity=\frac{0.063 moles}{0.05 L}

Molarity= 1.26 \frac{ moles}{L}

<u><em>The molarity is 1.26 </em></u>\frac{ moles}{L}<u><em></em></u>

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