What is the Molarity of a solution containing 432 grams of Ca(NO3)2 in 6.7 liters of water?Group of answer choices0.428 M0.298 M0.393 M.352 M
Question
What is the Molarity of a solution containing
432 grams of Ca(NO3)2 in 6.7 liters of water?
Group of answer choices
0.428 M
0.298 M
0.393 M
0.352 M
Solution
To find the molarity of the solution, we need to follow these steps:
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First, we need to find the molar mass of Ca(NO3)2. The molar mass of Ca(NO3)2 is approximately 164 g/mol (40.08 g/mol for Ca, 28.01 g/mol for N, and 16.00 g/mol for O, multiplied by 6 because there are 6 oxygen atoms in the formula).
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Next, we divide the mass of the solute by its molar mass to find the number of moles. So, 432 g ÷ 164 g/mol = 2.634 moles of Ca(NO3)2.
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Then, we divide the number of moles by the volume of the solution in liters to find the molarity. So, 2.634 moles ÷ 6.7 L = 0.393 M.
So, the molarity of the solution is 0.393 M.
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