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Calculate the freezing point of a solution containing 8.1 g of HBr in 100 g of water, assuming the acid to be 90 % ionized. [Given: Molar mass Br = 80 g/mol, Kf water = 1.86 K kg / mol]?
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Calculate the freezing point of a solution containing 8.1 g of HBr in ...
Step 1: Calculate Moles of HBr
To find the moles of HBr in the solution, we first need to determine its molar mass:
- Molar mass of H = 1 g/mol
- Molar mass of Br = 80 g/mol
- Molar mass of HBr = 1 + 80 = 81 g/mol
Now, calculate the moles of HBr:
- Moles of HBr = mass / molar mass
- Moles of HBr = 8.1 g / 81 g/mol = 0.1 mol
Step 2: Calculate Ionization
Since HBr is 90% ionized:
- Ionized HBr = 0.1 mol × 0.90 = 0.09 mol
- Total particles (considering it dissociates into H⁺ and Br⁻):
Total = 0.09 mol H⁺ + 0.09 mol Br⁻ = 0.18 mol
Step 3: Calculate Molality
To find molality (m):
- Mass of water = 100 g = 0.1 kg
- Molality (m) = moles of solute / mass of solvent (kg)
- m = 0.18 mol / 0.1 kg = 1.8 mol/kg
Step 4: Calculate Freezing Point Depression
Using the formula for freezing point depression:
- ΔTf = Kf × m
- ΔTf = 1.86 K kg/mol × 1.8 mol/kg = 3.348 K
Step 5: Calculate Freezing Point of the Solution
The freezing point of pure water is 0°C. Therefore:
- Freezing point of solution = 0°C - ΔTf
- Freezing point of solution = 0°C - 3.348 K = -3.348°C
Final Result
The freezing point of the solution containing 8.1 g of HBr in 100 g of water, assuming 90% ionization, is approximately -3.35°C.
Community Answer
Calculate the freezing point of a solution containing 8.1 g of HBr in ...
-3.534 degree Celsius
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Calculate the freezing point of a solution containing 8.1 g of HBr in 100 g of water, assuming the acid to be 90 % ionized. [Given: Molar mass Br = 80 g/mol, Kf water = 1.86 K kg / mol]?
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