In: Chemistry
Benzoic Acid and TBA
Finish the given table:
Trial 1 Trial 2
1. Kf for TBA 9.1° C/m 9.1° C/m
2. Mass of Benzoic Acid (g) 1.01 g 1.01 g
3. Freezing point of benzoic Acid
and TBA solution from graph 20.4 C 17.6 C
4. Freezing point change 3.8°C 2.6° C
5. Molality of solution ? ?
6. Calculated molar mass of Benzoic Acid (g/mol) ? ?
7. Average Molar Mass (g/mol) ? ?
8. Standard Deviation ?
9. Relative Standard Deviation ?
Trial 1:
molality = mol of solute / kg of solvent
or, form colligative properties
dTf = -Kf*m
where dTf = depression point of mixture
Kf = constant of solvent
m = molality of solvent
so
m = dTf/Kf = 3.8°C/9.1°C/m= 0.41758 molal
Q6.
calculated MM of B.A = mass/mol
we have mass = 1.01g but not moles
mass of solvent --> 19.805 g of solvent
claculate mass
mol of S = molality * kg solvent= (0.41758 )(19.805 /1000) = 0.0082701 mol of S
so
MM = mass / mol = 1.01/0.0082701 = 122.1266 g/mol
Trial 2:
molality = mol of solute / kg of solvent
or, form colligative properties
dTf = -Kf*m
where dTf = depression point of mixture
Kf = constant of solvent
m = molality of solvent
so
m = dTf/Kf = 2.6°C/9.1°C/m= 0.28571 molal
Q6.
calculated MM of B.A = mass/mol
we have mass = 1.01g but not moles
mass of solvent --> 19.805 g of solvent
claculate mass
mol of S = molality * kg solvent= (0.28571)(19.805 /1000) = 0.0056584mol of S
so
MM = mass / mol = 1.01/0.0056584= 178.4 g/mol
Q7.
average...
MW = (178.4+122.1266 )/2 = 150.2633 g/mol
Q8.
STDdev = sqrt(178.4-150.2633)^2 (122.1266 -150.2633g)^2) = 39.79130 g/moll
Std. dev ---> 39.79130/150.2633 = 0.2648 (unitless)