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Alisiya [41]
4 years ago
9

Calcium chloride, CaCl2, is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. A sol

ution is made by adding 6.50 g of CaCl2 to 60.0 mL of water at 25∘C. The density of the solvent at that temperature is 0.997 g/mL. Calculate the mole percent of CaCl2 in the solution.
Chemistry
1 answer:
zhannawk [14.2K]4 years ago
5 0

Answer:

Mole percent of CaCl_{2} in solution is 1.71%

Explanation:

Number of moles of a compound is the ratio of mass to molar mass of the compound.

Molar mass of CaCl_{2} = 110.98 g/mol

Molar mass of H_{2}O = 18.02 g/mol

Density is the ratio of mass to volume

So, mass of 60.0 mL of water = (60\times 0.997)g=60.8g

Hence, 6.50 g of CaCl_{2} = \frac{6.50}{110.98}moles of CaCl_{2} = 0.0586 moles of CaCl_{2}

60.8 g of H_{2}O= \frac{60.8}{18.02}moles of H_{2}O = 3.37 moles of H_{2}O

So, mole percent of CaCl_{2} in solution = \frac{n_{CaCl_{2}}}{n_{total}}\times 100% = \frac{0.0586}{0.0586+3.37}\times 100% = 1.71%

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