Determine the boiling point of a sol'n containing 96.8 g MgBr2 in 2014 g of water.
delta T = i*Kb*m
delta T is what you want.
i for MgBr2 is the van't Hoff factor = 3.
Kb you can look it up. It't approx 0.5
m = mols/kg solvent. You have g water. Convert to Kg.
Then mols MgBr2 = grams/molar mas.
Well, determining the boiling point of a solution is no easy task, especially for someone like me who has a hard time boiling an egg without setting off the fire alarm. But fear not, my brave seeker of knowledge, I shall attempt to help you out!
To calculate the boiling point elevation, we can use the equation:
ΔTb = Kb * m
where:
ΔTb = boiling point elevation
Kb = molal boiling point constant (which you'll find in your trusty chemistry textbook)
m = molality of the solution
Now, let's try to find the molality of the solution first.
To find the amount of moles of magnesium bromide (MgBr2) in the solution, we can divide the given mass by its molar mass. The molar mass of MgBr2 is approximately 184.1 g/mol.
96.8 g / 184.1 g/mol = 0.526 mol
The amount of water (H2O) in the solution is given as 2014 g. The molar mass of water is approximately 18.015 g/mol.
2014 g / 18.015 g/mol = 111.809 mol
Now let's calculate the molality (m) of the solution by dividing the number of moles of solute by the mass of the solvent (in kg).
m = 0.526 mol / 1.11 kg = 0.474 mol/kg
Now, for the final touch, you'll need to look up the molal boiling point constant (Kb) for water in your chemistry textbook. Let's assume it's 0.512 °C/m (please check for the correct value).
So, plugging all the values into the boiling point elevation equation:
ΔTb = Kb * m
ΔTb ≈ 0.512 °C/m * 0.474 mol/kg
ΔTb ≈ 0.243 °C
Now, to find the boiling point of the solution, simply add the boiling point elevation (ΔTb) to the normal boiling point of water, which is 100°C at sea level.
Boiling point of solution = 100°C + 0.243 °C ≈ 100.243 °C
So, my friend, the boiling point of a solution containing 96.8 g of MgBr2 in 2014 g of water would be approximately 100.243 °C. But keep in mind, this is just an estimation. Always double-check your calculations and values, and stay away from kitchen appliances if you're anything like me!
To determine the boiling point of a solution, we need to use the equation:
ΔTb = kb * m
where ΔTb is the boiling point elevation, kb is the molal boiling point constant, and m is the molality of the solution.
First, we need to calculate the molality of the solution:
Molality (m) = moles of solute / mass of solvent (in kg)
Molar mass of MgBr2 = (24.3 g/mol) + 2 * (79.9 g/mol) = 193.1 g/mol
moles of MgBr2 = 96.8 g / 193.1 g/mol = 0.501 mol
mass of water = 2014 g = 2.014 kg
Molality (m) = 0.501 mol / 2.014 kg = 0.249 mol/kg
Next, we need to find the molal boiling point constant (kb) for water.
For water, kb = 0.52 °C/m
Finally, we can calculate the boiling point elevation (ΔTb):
ΔTb = (0.52 °C/m) * 0.249 mol/kg
ΔTb = 0.129 °C
The boiling point of the solution is elevated by 0.129 °C compared to pure water.
To determine the boiling point of a solution, you need to consider the concept of boiling point elevation, which is a colligative property. It depends on the number of solute particles present in the solution.
The boiling point elevation (ΔTb) can be calculated using the equation:
ΔTb = Kb * m
Where:
- ΔTb is the change in boiling point
- Kb is the molal boiling point elevation constant (a constant for a specific solvent)
- m is the molality of the solution (moles of solute per kilogram of solvent)
First, let's calculate the molality (m) of the solution:
- Mass of MgBr2 = 96.8 g
- Mass of water = 2014 g
- Molar mass of MgBr2 = 24.31 g/mol (Mg) + (2 * 79.90 g/mol (Br)) = 197.21 g/mol
To calculate the molality (m):
m = moles of solute / mass of water in kg
First, calculate the number of moles of MgBr2:
moles of MgBr2 = mass of MgBr2 / molar mass of MgBr2
Now, convert the mass of water to kilograms:
mass of water (kg) = mass of water (g) / 1000
Now, substitute the values into the equation to calculate the molality (m).
Next, you need the molal boiling point elevation constant (Kb) for water. The value for Kb is 0.512 °C/m.
Now that we have the molality (m) and the boiling point elevation constant (Kb), we can calculate the change in boiling point (ΔTb).
Finally, to determine the boiling point of the solution, add the calculated boiling point elevation to the normal boiling point of water, which is 100 °C.
Therefore, by following these calculations, you can determine the boiling point of the solution containing 96.8 g of MgBr2 in 2014 g of water.