A 2.00 g samples of benzoic acid (mw = 122.2 amu) is dissolved in 50.0 g of lauric acid acid, which has a normal melting point of 45.0 oC. If the new solution has a depressed freezing point of 43.7 oC, what is the freezing point depression constant for lauric acid?
A.0.251 oC/m
B.3.97 oC/m *
C.3.25 oC/m
D.0.307 oC/m
E.None of the above
A 2.00 g samples of benzoic acid (mw = 122.2 amu) is dissolved in 50.0 g...
DATA AND CALCULATIONS Mass of lauric acid Mass of benzoic acid Freezing temperature of pure lauric acid Freezing point of the benzoic acid-lauric acid mixture Freezing temperature depression, At 38-1c Molality, m molkg Moles of benzoic acid mol Molecular weight of benzoic acid (experimental) g/mo Molecular weight of benzoic acid (accepted) g/mol Percent error
DATA TABLE Mass of lauric acid (9) 8.25 1.09 42.22 C Mass of benzoic acid (g) Freezing temperature of pure lauric acid ('C) Freezing point of the benzoic acid-lauric acid mixture (C)39,11°c Going Further Questions: 1. Calculate molality (m), in molkg, using the formula AT- Kx m. The K value for lauric acid is 3.9°c-kg/mol. 2. Calculate moles of benzoic acid solute, using the molality and the mass (in kg) of lauric acid solvent. 3. Calculate the experimental molecular weight...
A sample of 4.6434 g of benzoic acid, C_7H_6O_2, is dissolved in 50.0033 g of camphor. what is the freezing point of the resulting solution? For camphor, T_f = 179.5 degree C, K_f = 40.00 degree C/m.
A solution of 1.5 g benzoic acid (C6H5COOH; MW = 122.123 g/mol) in 100.0 g of carbon tetrachloride (CCl4; MW =153.822 g/mol) has a boiling point of 77.50°C. The boiling point of pure carbon tetrachloride is 76.72°C and the melting point is -22.92°C. Calculate the molecular weight of benzoic acid in the solution. Suggest a reason for the difference between the molar mass based on the formula (listed above) and the molar mass determined in part a.
When 0.3163 g of benzoic acid (C7H6O2) was dissolved in 15.563 g cyclohexanol, the freezing point of the mixture was 8.19 degrees C lower than that of the pure cyclohexanol. What is the molal freezing point constnt of the cyclohexanol? (delta T = m x Kf x i)
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water to produce a 50.0 mL solution. The pH of this solution is measure to be pH = 2.13. Determine the ionization constant (Ka) of the acid. 8. A buffer is 0.50 M CH3COOH(aq) and 0.50 M Na(C6H-C00) (aq). For CH2COOH pKa = 4.20 a) Calculate the pH of the buffer solution. b) Calculate the pH after the addition of 40 mL of a 0.150...
12.22 g of the monoprotic acid KHP(MW = 204.2 g/mol) is dissolved into water. The sample is titrated with a 0.85 M solution of calcium hydroxide to the equivalence point. What volume of base was used?
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an end point with 24.80 mL of 0.629 M Cr2O72−. The following redox reaction takes place: Cr2O72− (aq) + Fe2+ (aq) ⟶ Cr3+ (aq) + Fe3+ (aq) a. balance the reaction b. what % of the ore sample if FeBr2 (molar mass = 215.65 g/mol)