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Chapter 12: Problem 200

What is the mass in grams of the nitrogen atoms in \(100.0 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) solution?

Short Answer

Expert verified
The mass of nitrogen atoms in \(100.0 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{Ca}(\mathrm{NO}_{3})_{2}\) solution is 2.802 grams.

Step by step solution

01

Calculate the moles of Ca(NO3)2

To calculate the number of moles of Ca(NO3)2 in solution, we will use the given molarity and volume of the solution: Moles of Ca(NO3)2 = Molarity × Volume Given, Molarity = 1.00 M Volume = 100.0 mL (Converted to liters, 0.100 L) Moles of Ca(NO3)2 = 1.00 M × 0.100 L = 0.100 mol
02

Determine the moles of nitrogen atoms

In the formula for calcium nitrate, Ca(NO3)2, there are 2 nitrate (NO3) ions per formula unit. Since there is one nitrogen atom in each nitrate, this means there are 2 nitrogen atoms per formula unit of Ca(NO3)2. Therefore, the number of moles of nitrogen atoms will be twice the number of moles of Ca(NO3)2. Moles of nitrogen atoms = Moles of Ca(NO3)₂ × 2 Moles of nitrogen atoms = 0.100 mol × 2 = 0.200 mol
03

Convert moles of nitrogen atoms into grams

Finally, to find the mass of nitrogen atoms in grams, we will use the molar mass of nitrogen and the number of moles calculated in step 2: Mass = Moles × Molar Mass Molar Mass of nitrogen = 14.01 g/mol (from the periodic table) Mass of nitrogen atoms = 0.200 mol × 14.01 g/mol = 2.802 g So, the mass of nitrogen atoms in 100.0 mL of 1.00 M Ca(NO3)2 solution is 2.802 grams.

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