A coordination compound is composed of 20.5 % Co, 19.5 % N, 37.0 % Cl, 6.3 % H,and 16.7 % O. It reacts with AgNO3 yielding 2 moles AgCl per mole of thecompound. It loses 2 moles of water on mild heating. It does not react with HCl. Itsconductivity is equivalent two 3 moles ion per mole of compound. Write theformula of the complex and name it.
Question
A coordination compound is composed of 20.5 % Co, 19.5 % N, 37.0 % Cl, 6.3 % H,and 16.7 % O. It reacts with AgNO3 yielding 2 moles AgCl per mole of thecompound. It loses 2 moles of water on mild heating. It does not react with HCl. Itsconductivity is equivalent two 3 moles ion per mole of compound. Write theformula of the complex and name it.
Solution
To determine the formula of the complex and name it, we need to analyze the given information step by step.
Step 1: Calculate the molar masses of each element in the compound.
- Co (cobalt) has a molar mass of 58.93 g/mol.
- N (nitrogen) has a molar mass of 14.01 g/mol.
- Cl (chlorine) has a molar mass of 35.45 g/mol.
- H (hydrogen) has a molar mass of 1.01 g/mol.
- O (oxygen) has a molar mass of 16.00 g/mol.
Step 2: Calculate the number of moles of each element in the compound.
- Co: (20.5 g / 58.93 g/mol) = 0.348 mol
- N: (19.5 g / 14.01 g/mol) = 1.39 mol
- Cl: (37.0 g / 35.45 g/mol) = 1.04 mol
- H: (6.3 g / 1.01 g/mol) = 6.24 mol
- O: (16.7 g / 16.00 g/mol) = 1.04 mol
Step 3: Determine the empirical formula of the compound. To find the empirical formula, we need to divide the number of moles of each element by the smallest number of moles. In this case, the smallest number of moles is 0.348 mol (from Co).
- Co: 0.348 mol / 0.348 mol = 1
- N: 1.39 mol / 0.348 mol = 4
- Cl: 1.04 mol / 0.348 mol = 3
- H: 6.24 mol / 0.348 mol = 18
- O: 1.04 mol / 0.348 mol = 3
Therefore, the empirical formula of the compound is CoN4Cl3H18O3.
Step 4: Determine the molecular formula of the compound. To find the molecular formula, we need to know the molar mass of the compound. Let's assume the molar mass is M.
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Empirical formula molar mass: (1 * 58.93 g/mol) + (4 * 14.01 g/mol) + (3 * 35.45 g/mol) + (18 * 1.01 g/mol) + (3 * 16.00 g/mol) = 342.79 g/mol
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Given molar mass: 342.79 g/mol
To find the molecular formula, we divide the given molar mass by the empirical formula molar mass.
- Molecular formula: (342.79 g/mol) / (342.79 g/mol) = 1
Therefore, the molecular formula of the compound is the same as the empirical formula, which is CoN4Cl3H18O3.
Step 5: Name the complex. Based on the formula, the complex contains cobalt (Co) as the central metal ion. The ligands are nitrogen (N), chlorine (Cl), hydrogen (H), and oxygen (O). To name the complex, we need to identify the ligands and their charges.
- Nitrogen (N) is a neutral ligand.
- Chlorine (Cl) is a negatively charged ligand with a charge of -1.
- Hydrogen (H) is a positively charged ligand with a charge of +1.
- Oxygen (O) is a neutral ligand.
The complex contains 4 nitrogen ligands, 3 chlorine ligands, 18 hydrogen ligands, and 3 oxygen ligands. Based on this information, the name of the complex is:
Tetraamminechloridotrihydroxocobalt(III) chloride.
Note: The Roman numeral (III) indicates the oxidation state of cobalt.
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