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Sagot :
To determine which solute raises the boiling point of water the most, we need to understand the concept of boiling point elevation, which is a colligative property. This means that the boiling point elevation depends on the number of particles in solution rather than the specific type of particles.
Here’s a step-by-step analysis:
1. Molecular Sucrose [tex]$\left(C_{12}H_{22}O_{11}\right)$[/tex]:
- Sucrose is a molecular compound and does not dissociate in water.
- It remains as a single molecule: \(C_{12}H_{22}O_{11} \rightarrow C_{12}H_{22}O_{11}\).
- Number of particles in solution: 1 molecule.
2. Ionic Sodium Chloride [tex]$(NaCl)$[/tex]:
- Sodium chloride is an ionic compound and dissociates completely in water.
- \(NaCl \rightarrow Na^+ + Cl^-\).
- Number of particles in solution: 2 ions (one \(Na^+\) and one \(Cl^-\)).
3. Ionic Potassium Bromide [tex]$(KBr)$[/tex]:
- Potassium bromide is an ionic compound and dissociates completely in water.
- \(KBr \rightarrow K^+ + Br^-\).
- Number of particles in solution: 2 ions (one \(K^+\) and one \(Br^-\)).
4. Ionic Calcium Chloride [tex]$\left(CaCl_2\right)$[/tex]:
- Calcium chloride is an ionic compound and dissociates completely in water.
- \(CaCl_2 \rightarrow Ca^{2+} + 2Cl^-\).
- Number of particles in solution: 3 ions (one \(Ca^{2+}\) and two \(Cl^-\)).
5. Ionic Aluminum Fluoride [tex]$\left(AlF_3\right)$[/tex]:
- Aluminum fluoride is an ionic compound and dissociates completely in water.
- \(AlF_3 \rightarrow Al^{3+} + 3F^-\).
- Number of particles in solution: 4 ions (one \(Al^{3+}\) and three \(F^-\)).
Boiling point elevation is proportional to the number of particles in the solution. More particles mean a greater elevation in the boiling point.
- Sucrose: 1 particle
- Sodium Chloride: 2 particles
- Potassium Bromide: 2 particles
- Calcium Chloride: 3 particles
- Aluminum Fluoride: 4 particles
As we can see, aluminum fluoride [tex]$\left(AlF_3\right)$[/tex] produces the highest number of particles, 4 ions per formula unit.
Thus, ionic aluminum fluoride [tex]$\left(AlF_3\right)$[/tex] raises the boiling point of water the most.
The correct answer is:
[tex]\[ \text{E. ionic aluminum fluoride } (AlF_3) \][/tex]
Here’s a step-by-step analysis:
1. Molecular Sucrose [tex]$\left(C_{12}H_{22}O_{11}\right)$[/tex]:
- Sucrose is a molecular compound and does not dissociate in water.
- It remains as a single molecule: \(C_{12}H_{22}O_{11} \rightarrow C_{12}H_{22}O_{11}\).
- Number of particles in solution: 1 molecule.
2. Ionic Sodium Chloride [tex]$(NaCl)$[/tex]:
- Sodium chloride is an ionic compound and dissociates completely in water.
- \(NaCl \rightarrow Na^+ + Cl^-\).
- Number of particles in solution: 2 ions (one \(Na^+\) and one \(Cl^-\)).
3. Ionic Potassium Bromide [tex]$(KBr)$[/tex]:
- Potassium bromide is an ionic compound and dissociates completely in water.
- \(KBr \rightarrow K^+ + Br^-\).
- Number of particles in solution: 2 ions (one \(K^+\) and one \(Br^-\)).
4. Ionic Calcium Chloride [tex]$\left(CaCl_2\right)$[/tex]:
- Calcium chloride is an ionic compound and dissociates completely in water.
- \(CaCl_2 \rightarrow Ca^{2+} + 2Cl^-\).
- Number of particles in solution: 3 ions (one \(Ca^{2+}\) and two \(Cl^-\)).
5. Ionic Aluminum Fluoride [tex]$\left(AlF_3\right)$[/tex]:
- Aluminum fluoride is an ionic compound and dissociates completely in water.
- \(AlF_3 \rightarrow Al^{3+} + 3F^-\).
- Number of particles in solution: 4 ions (one \(Al^{3+}\) and three \(F^-\)).
Boiling point elevation is proportional to the number of particles in the solution. More particles mean a greater elevation in the boiling point.
- Sucrose: 1 particle
- Sodium Chloride: 2 particles
- Potassium Bromide: 2 particles
- Calcium Chloride: 3 particles
- Aluminum Fluoride: 4 particles
As we can see, aluminum fluoride [tex]$\left(AlF_3\right)$[/tex] produces the highest number of particles, 4 ions per formula unit.
Thus, ionic aluminum fluoride [tex]$\left(AlF_3\right)$[/tex] raises the boiling point of water the most.
The correct answer is:
[tex]\[ \text{E. ionic aluminum fluoride } (AlF_3) \][/tex]
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