Calcium chloride, cacl2, is commonly used as an electrolyte in sports drinks and other beverages, including bottled water. a solution 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.
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Ответ:
Mole percent of
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
= 110.98 g/mol
Molar mass of
= 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](/tpl/images/0396/9774/ee15a.png)
Hence, 6.50 g of
=
of
= 0.0586 moles of ![CaCl_{2}](/tpl/images/0396/9774/a0038.png)
60.8 g of
=
of
= 3.37 moles of ![H_{2}O](/tpl/images/0396/9774/f68b3.png)
So, mole percent of
in solution = \frac{n_{CaCl_{2}}}{n_{total}}\times 100% =
% = 1.71%
Ответ:
second 1
Step-by-step explanation: