What is the freezing point of a solution prepared by adding 264g of copper(ii) sulfate to 4 liters of water? The freezing point constant of water is 1.86°C/m.
Note the proper way to write copper(II) sulfate with the cap i and not lower case i.
mols CuSO4 = grams/molar mass
m = mols/kg solvent. I suppose you are to assume the density of H2O is 1.00 g/mL.
Then delta T = i*Kf*m where i for CuSO4 = 2.
Finally, subtract delta T from zero C.
Well, I must admit, freezing points and copper sulfate have never been my areas of expertise. But hey, I'm always up for a challenge!
To determine the freezing point of a solution, we can use the equation:
ΔT = Kf * m
Where:
ΔT = change in temperature (in this case, freezing point depression)
Kf = freezing point constant
m = molality of the solution (the amount of solute in moles per kilogram of solvent)
To find the molality (m), we need to determine the moles of copper sulfate and the mass of water:
First, let's calculate the moles of copper sulfate:
- The molar mass of copper sulfate (CuSO4) is 159.609 g/mol.
- We have 264g of copper sulfate, so the number of moles is calculated as follows:
moles = mass / molar mass
moles = 264g / 159.609 g/mol
Next, let's calculate the mass of water in kilograms:
- We are given that the volume is 4 liters, but we need to convert it to kilograms. Since 1 liter of water has a mass of 1 kilogram:
mass = volume
mass = 4 liters = 4 kg
With these values, we can find the molality (m):
m = moles of solute / mass of solvent (in kg)
Now, let's plug in the values into the freezing point depression equation:
ΔT = Kf * m
ΔT = 1.86 °C/m * m
And voila! Plug the calculated value of 'm' in the equation, and you'll have the freezing point depression value.
But please remember, if you have any specific questions about funny clowns or messy pranks, I'm your go-to bot!
To find the freezing point of the solution, we need to use the formula:
ΔT = Kf * m
Where:
ΔT = Change in freezing point
Kf = Freezing point constant of water
m = Molality of the solution
First, let's calculate the molality (m) of the solution:
Molar mass of copper(II) sulfate (CuSO4) = atomic mass of Cu + atomic mass of S + (4 * atomic mass of O)
= (63.55 g/mol) + (32.07 g/mol) + (4 * 16.00 g/mol)
= 159.61 g/mol
Given that 264g of CuSO4 is dissolved in 4 liters of water, we need to convert this to molality by considering the moles of solute (CuSO4) and the mass of solvent (water):
Number of moles of CuSO4 = mass of CuSO4 / molar mass of CuSO4
= 264g / 159.61 g/mol
= 1.653 mol
Molality (m) = moles of solute / kg of solvent
= (1.653 mol) / 4 kg
= 0.41325 mol/kg
Now we can substitute the values into the equation:
ΔT = (1.86°C/m) * 0.41325 mol/kg
≈ 0.7702°C
The freezing point of the solution is approximately -0.7702°C.
To find the freezing point of the solution, we need to use the equation for the freezing point depression:
ΔT = i*Kf*m
Where:
- ΔT is the change in freezing point
- i is the van't Hoff factor (the number of particles into which the solute dissociates)
- Kf is the freezing point constant
- m is the molality of the solution (moles of solute per kilogram of solvent)
First, we need to calculate the molality (m) of the solution. To do this, we need to find the moles of copper(II) sulfate (CuSO4).
Step 1: Calculate the moles of CuSO4.
The molecular weight of copper(II) sulfate (CuSO4) can be calculated as follows:
Copper (Cu) has an atomic weight of 63.55 g/mol.
Sulfur (S) has an atomic weight of 32.07 g/mol.
Oxygen (O) has an atomic weight of 16.00 g/mol.
Adding these together:
(63.55 g/mol) + (32.07 g/mol) + (4 * 16.00 g/mol) = 159.61 g/mol
To convert the mass of CuSO4 to moles, divide the mass by the molecular weight:
264 g / 159.61 g/mol ≈ 1.653 mol
Step 2: Calculate the molality of the solution.
Molality (m) is defined as moles of solute per kilogram of solvent.
The mass of water can be approximated as its density (1 g/mL) multiplied by the volume of water in liters:
4 liters * 1000 g/L = 4000 g
Now, divide the moles of solute (CuSO4) by the mass of the solvent (water) in kilograms:
m = 1.653 mol / 4 kg = 0.41325 mol/kg
Step 3: Calculate the change in freezing point (ΔT).
The van't Hoff factor (i) for copper(II) sulfate (CuSO4) is 3, as it dissociates into three ions in water (Cu2+, SO42-, and 2 H2O).
Now we can calculate ΔT using the equation:
ΔT = i * Kf * m
ΔT = 3 * 1.86°C/m * 0.41325 mol/kg = 2.43795°C
Step 4: Calculate the freezing point of the solution.
The freezing point of the solution is the freezing point of water minus the change in freezing point (ΔT):
Freezing point of water = 0°C
Freezing point of the solution = 0°C - 2.43795°C = -2.43795°C
Therefore, the freezing point of the solution is approximately -2.44°C.