put in decreasing freezing point 0.10m Na3PO4,0.35m NaCl,0.20 m MgCl2, 0.15 m C6H12O6,0.15 m CH3COOH
delta T = i*Kf*m
Since Kf is a constant you may ignore it and multiply i*m. The largest number will be the largest delta T.
Arrenge Na3PO4 m, 0.35 m NaCl,0.2m MgCl2m,0.15m C6H12O6 m, 0.15CH3COOH m in decreasing order of their expected freezing point
To determine the order of decreasing freezing points for the given solutions, we need to consider their respective concentrations and the number of particles they dissociate into.
1. Na3PO4:
Na3PO4 dissociates into 3 ions - 3 Na+ ions and 1 PO4^3- ion. So, it will have the largest effect on the freezing point depression among the given solutions.
2. NaCl:
NaCl dissociates into 2 ions - 1 Na+ ion and 1 Cl- ion.
3. MgCl2:
MgCl2 dissociates into 3 ions - 1 Mg^2+ ion and 2 Cl- ions.
4. C6H12O6:
C6H12O6 does not dissociate into ions since it is a non-electrolyte. Therefore, it will have the least effect on the freezing point depression.
5. CH3COOH:
CH3COOH (acetic acid) partially dissociates into ions but in this case, we'll consider it as a non-electrolyte to simplify the comparison.
Based on the above information, the solutions in decreasing order of their freezing points would be:
1. Na3PO4 (0.10 m)
2. MgCl2 (0.20 m)
3. NaCl (0.35 m)
4. CH3COOH (0.15 m)
5. C6H12O6 (0.15 m)
Please note that the freezing point depression also depends on other factors like the solute-solvent interactions and the nature of the solute itself.
To determine the decreasing order of freezing points for the given solutions, we need to consider the concept of freezing point depression.
Freezing point depression is a colligative property, which means that it depends on the number of solute particles and not their nature. According to the colligative property, the freezing point of a solution is lower than that of the pure solvent.
The formula to calculate the freezing point depression is:
ΔT = Kf * m * i
Where:
- ΔT represents the change in freezing point
- Kf is the cryoscopic constant (freezing point depression constant) for the solvent
- m is the molality of the solution (moles of solute per kilogram of solvent)
- i is the van't Hoff factor, which represents the number of particles formed from each solute molecule in the solution. For ionic compounds, i is equal to the number of ions produced when the compound dissociates.
Let's calculate the freezing point depression (ΔT) for each solution and compare them:
1. 0.10m Na3PO4:
- As Na3PO4 dissociates into four ions (3Na+ and PO4^-3), i = 4.
- Find the value of Kf for the solvent being used.
- Calculate ΔT using the given molality (m) and the calculated values of Kf and i.
2. 0.35m NaCl:
- NaCl dissociates into two ions (Na+ and Cl-), so i = 2.
- Calculate ΔT using the given molality (m) and the Kf value.
3. 0.20m MgCl2:
- MgCl2 dissociates into three ions (Mg^2+ and 2Cl-), so i = 3.
- Calculate ΔT using the given molality (m) and the Kf value.
4. 0.15m C6H12O6:
- C6H12O6 is a molecular compound and does not dissociate, so i = 1.
- Calculate ΔT using the given molality (m) and the Kf value.
5. 0.15m CH3COOH:
- CH3COOH is a molecular compound and does not dissociate significantly, so i may be approximated as 1.
- Calculate ΔT using the given molality (m) and the Kf value.
After calculating the ΔT values for each solution, we can compare them to determine the decreasing order of freezing points. The solution with the highest magnitude of ΔT will have the lowest freezing point.
Note: To provide a specific answer, the values for Kf and the associated solvent are required. This information is generally provided in the context of the problem or experiment.