Assuming equal concentration rank these by freezing points, Na3PO4, Li2Co3,NH4Cl, and Sn(NO3)4
delta T = i*Kf*m
Since Kf and m are the same for all of these it will depend upon i, the van't Hoff factor.
i = 4 for Na3PO4
i = 3 for Li2CO3.
i = 2 for NH4Cl
i = 5 for Sn(NO3)4
To rank the given compounds by their freezing points, we need to consider the nature of the ions present in each compound. The freezing point of a solution is influenced by factors such as the number of particles present, their charges, and their interactions.
Here's a step-by-step approach to determine the order of freezing points:
1. Identify the dissociation of each compound: Each compound will dissociate into ions when dissolved in water. Knowing the ions formed will help us determine the number of particles present.
a. Na3PO4 dissociates into 3 Na+ ions and 1 PO43- ion.
b. Li2CO3 dissociates into 2 Li+ ions and 1 CO32- ion.
c. NH4Cl dissociates into 1 NH4+ ion and 1 Cl- ion.
d. Sn(NO3)4 dissociates into 1 Sn4+ ion and 4 NO3- ions.
2. Understand the impact of the ions on freezing point: Generally, the more particles present in a solution, the lower the freezing point. This is known as the colligative property. Also, the charges of the ions can influence the strength of their interactions, affecting the freezing point.
3. Determine the number of particles in each compound: Based on the dissociation, count the total number of ions present.
a. Na3PO4 dissociates into 4 ions (3Na+ + 1PO43-).
b. Li2CO3 dissociates into 3 ions (2Li+ + 1CO32-).
c. NH4Cl dissociates into 2 ions (1NH4+ + 1Cl-).
d. Sn(NO3)4 dissociates into 5 ions (1Sn4+ + 4NO3-).
4. Compare the number of particles and charges: Since the concentrations are equal, we can infer that the freezing point depends on the total number of particles. The compound with the highest number of particles will have the lowest freezing point.
Ranking the compounds in order of their freezing points:
1. Sn(NO3)4 (5 ions)
2. Na3PO4 (4 ions)
3. Li2CO3 (3 ions)
4. NH4Cl (2 ions)
Therefore, the ranking of the compounds from the highest to the lowest freezing point is Sn(NO3)4, Na3PO4, Li2CO3, and NH4Cl.
To rank these compounds based on their freezing points, we need to consider their composition and the effect it has on the intermolecular forces.
1. NH4Cl (Ammonium chloride):
NH4Cl is an ionic compound consisting of ammonium ions (NH4+) and chloride ions (Cl-). Due to the strong electrostatic attraction between these ions, NH4Cl has a relatively high freezing point. Therefore, NH4Cl has the highest freezing point among the given compounds.
2. Na3PO4 (Sodium phosphate):
Na3PO4 is also an ionic compound, composed of sodium ions (Na+) and phosphate ions (PO4^3-). Similar to NH4Cl, the strong ionic bonding in Na3PO4 results in a higher freezing point compared to the remaining compounds.
3. Sn(NO3)4 (Tin(IV) nitrate):
Sn(NO3)4 is a molecular compound, containing tin(IV) ions (Sn4+) and nitrate ions (NO3-). The intermolecular forces in molecular compounds, such as Sn(NO3)4, are generally weaker than those in ionic compounds. Therefore, Sn(NO3)4 has a lower freezing point compared to NH4Cl and Na3PO4.
4. Li2Co3 (Lithium carbonate):
Li2Co3 is an ionic compound, consisting of lithium ions (Li+) and carbonate ions (CO3^2-). Although ionic compounds generally have higher freezing points, compared to molecular compounds, the presence of lithium ions, which are highly polarizing, weakens the ion-ion attractions. As a result, Li2Co3 has the lowest freezing point among the given compounds.
Ranking the compounds based on their freezing points from highest to lowest:
1. NH4Cl
2. Na3PO4
3. Sn(NO3)4
4. Li2Co3