Question

Chlorisondamine chloride \(\left(\mathrm{C}_{14} \mathrm{H}_{20} \mathrm{Cl}_{6} \mathrm{N}_{2}\right)\) is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated with an excess of silver nitrate, 0.104 g silver chloride was recovered. Calculate the mass percent of chlorisondamine chloride in the medication, assuming the drug is the only source of chloride.

Short answer

Using the given information and following the steps above, we can calculate the mass percent of chlorisondamine chloride in the medication. 1. Calculate the mass of Chloride ions by using the mass of silver chloride: \(m_{\mathrm{Cl}} = \frac{(0.104\ \mathrm{g}) \times (35.45\ \mathrm{g/mol})}{143.32\ \mathrm{g/mol}} = 0.0253\ \mathrm{g}\) 2. Calculate the moles of Chloride ions: \(n_{\mathrm{Cl}} = \frac{0.0253\ \mathrm{g}}{35.45\ \mathrm{g/mol}} = 7.14 \times 10^{-4}\ \mathrm{mol}\) 3. Calculate the moles of chlorisondamine chloride: \(n_{\mathrm{drug}} = 7.14 \times 10^{-4}\ \mathrm{mol}\). 4. Calculate the mass of chlorisondamine chloride: \(m_{\mathrm{drug}} = (7.14 \times 10^{-4}\ \mathrm{mol}) \times (448.92\ \mathrm{g/mol}) = 0.320\ \mathrm{g}\) (molar mass of chlorisondamine chloride, \(M_{\mathrm{drug}} = 448.92\ \mathrm{g/mol}\)) 5. Calculate the mass percent of chlorisondamine chloride in the medication: \(\text{Mass Percent} = \frac{0.320\ \mathrm{g}}{1.28\ \mathrm{g}} \times 100 = 25.0\%\) The mass percent of chlorisondamine chloride in the medication is \(25.0\%\).

Step-by-step solution

Calculate the mass of Chloride ions in the sample

To do this, we will use the mass of the recovered silver chloride. The mass of silver chloride is given as 0.104 g. Using the molar mass of silver (\(Ag=107.87\) g/mol) and the molar mass of chloride (\(Cl=35.45\) g/mol), we can calculate the mass of Chloride ions in the sample. The mass of one mole of Silver chloride, \(\mathrm{AgCl}\) is \[ \mathrm{AgCl} = 107.87\ \mathrm{g/mol} + 35.45\ \mathrm{g/mol} = 143.32\ \mathrm{g/mol} \] Now, we can use the mass ratio of Chloride ions in one mole of silver chloride to find the mass of Chloride ions in the sample: \[ m_{\mathrm{Cl}} = \frac{m_{\mathrm{sample}} \times M_{\mathrm{Cl}}}{M_{\mathrm{AgCl}}} \] Where \(m_{\mathrm{Cl}}\) is the mass of Chloride ions, \(m_{\mathrm{sample}}\) is the mass of the sample in g, \(M_{\mathrm{Cl}}\) is the molar mass of chloride, and \(M_{\mathrm{AgCl}}\) is the molar mass of silver chloride.

Calculate the moles of Chloride ions in the sample

Now that we have found the mass of Chloride ions in the sample, we will use it to determine the number of moles: \[ n_{\mathrm{Cl}}=\frac{m_{\mathrm{Cl}}}{M_{\mathrm{Cl}}} \] Where \(n_{\mathrm{Cl}}\) is the moles of Chloride ions and \(m_{\mathrm{Cl}}\) and \(M_{\mathrm{Cl}}\) are the mass of Chloride ions and the molar mass of Chloride ions, respectively.

Calculate the moles of chlorisondamine chloride in the sample

Since there's a 1:1 relationship between the moles of Chloride ions and the moles of chlorisondamine chloride, the moles of Chloride ions will be equal to the moles of the chlorisondamine chloride: \[ n_{\mathrm{drug}} = n_{\mathrm{Cl}} \] Where \(n_{\mathrm{drug}}\) is the moles of chlorisondamine chloride and \(n_{\mathrm{Cl}}\) is the moles of Chloride ions.

Calculate the mass of chlorisondamine chloride in the sample

Using the moles of chlorisondamine chloride and its molecular formula \(\mathrm{C}_{14} \mathrm{H}_{20} \mathrm{Cl}_{6} \mathrm{N}_{2}\), we can find the mass of the drug: \[ m_{\mathrm{drug}} = n_{\mathrm{drug}} \times M_{\mathrm{drug}} \] Where \(m_{\mathrm{drug}}\) is the mass of chlorisondamine chloride, \(n_{\mathrm{drug}}\) is the moles of chlorisondamine chloride, and \(M_{\mathrm{drug}}\) is the molar mass of chlorisondamine chloride.

Calculate the mass percent of chlorisondamine chloride in the medication

Now, we can calculate the mass percent of chlorisondamine chloride in the medication using the mass of the drug and the mass of the sample: \[ \text{Mass Percent} = \frac{m_{\mathrm{drug}}}{m_{\mathrm{sample}}} \times 100 \] Where \(m_{\mathrm{drug}}\) is the mass of chlorisondamine chloride, and \(m_{\mathrm{sample}}\) is the mass of the sample.

Key concepts

Chloride Ion Analysis

When analyzing a sample to determine its chemical composition, especially in the context of chloride ions, it's important to release all chlorine-containing compounds as chloride ions. In this exercise, chlorisondamine chloride, present in a medication, is analyzed. The organic material within the medication is destroyed to ensure that the chlorine present converts entirely to chloride ions.

Once converted to chloride ions, they react with an excess of silver nitrate to form silver chloride, a precipitate. The amount of silver chloride formed directly correlates to the amount of chloride ions originally present. By measuring the mass of the silver chloride, we are able to back-calculate and find the mass of chloride ions. This process is central to our calculation of the mass percent of chlorisondamine chloride in the given sample.

Stoichiometry

Stoichiometry is a key concept in chemistry that involves quantitative relationships between reactants and products in chemical reactions. In this problem, we see stoichiometry in action when we look at the reactions between chloride ions and silver ions to form silver chloride.

In terms of stoichiometry:

• Every mole of chloride ion reacts with one mole of silver ion to produce one mole of silver chloride.
• This 1:1:1 molar ratio allows us to use the mass of silver chloride formed to determine the amount of chloride ion present.

By using stoichiometry, we can link the mass of the silver chloride back to the mass of chlorisondamine chloride, since we assume that all chloride ions originate from this drug.

Molar Mass Determination

Understanding molar mass is crucial when dealing with substances like chlorisondamine chloride and silver chloride. Molar mass allows chemists to convert between the mass of a substance and the number of moles, which is a common need in mass percent calculations.

In this exercise, we have:

• The molar mass of chloride is 35.45 g/mol.
• The molar mass of silver chloride (AgCl) is determined by adding the molar mass of silver (107.87 g/mol) and chloride (35.45 g/mol), giving 143.32 g/mol.

With these molar masses, we can calculate the moles of a substance from its mass, and vice versa. This step is essential for determining the mass and, subsequently, the mass percent of chlorisondamine chloride in the sample.

Chemical Reactions in Solutions

Chemical reactions in solutions are a fundamental part of this exercise. When the sample is processed, the reaction that primarily drives the analytical procedure involves the interaction between chloride ions released from chlorisondamine chloride and silver nitrate solution.

This reaction forms silver chloride precipitate: \[ \text{Ag}^{+} + \text{Cl}^{-} \rightarrow \text{AgCl} \]This precipitation reaction is a classic example of a double displacement reaction in solutions, where ions in the reacting solutions exchange places and form an insoluble product.

The formation of silver chloride is not only integral to the quantification of chloride ions but also assures the completion of chloride conversion from the sample. This progress was tracked by measuring the mass of the formed precipitate, which is then utilized in our calculation of chlorisondamine chloride content.