Calculate the molar mass of your unknown solute using the accepted literature Kf value of 8.3...
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Calculate the molar mass of your unknown solute using the accepted
literature Kf value of 8.3...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute...
Need help with freezing point depression expeiment volume of acetic acid 30 volume of unknown solute in solution1 1.5 volume of unknown solute in solution 2 1.5 freezing point of pure acetic acid 16.3 freezing point of solution 1 14.5 freezing point of solution 2 11.3 average molar mass of unknown solute Calculations for Part 1 The density of acetic acid is 1.049 g/mL and Kf(acetic acid) =3.90 °C·kg/mol The density of the unknown is 0.791 g/mL. 1.Calculate the masses...
Mass of lauric acid= 8.0021g Mass of unknown solute= 1.0036g Freexing temperature of pur lauric acid=42.62...
Mass of lauric acid= 8.0021g Mass of unknown solute= 1.0036g Freexing temperature of pur lauric acid=42.62 Freezing temperature point of the unknown solute and lauric acid =36.09 Calculate mole of benzoic acid solute, using the molality and the mass of lauric acid solvent Calculate the experimental molar mass of benzoic acid , in g/mol
Chemistry: Molar mass determination and freezing point depression. If your unknown solute sample weighed 0.634 grams,...
Chemistry:
Molar mass determination and freezing point depression.
If your unknown solute sample weighed 0.634 grams, but some of it stuck to the test tube wall when you were pouring it in and did not dissolve in the t-butyl alcohol, what sort of error will this cause in the calculated molar mass of your unknown solute? Explain. What would be the freezing point of an aqueous solution that contains 10.3 grams of ethylene glycol [(C_2H_4(OH)_2] in 100 mL of water?
Freezing Point Depression: Determination of the Molar Mass of an Unknown Substance Laboratory Record Unknown Identifier...
Freezing Point Depression: Determination of the Molar Mass of an Unknown Substance Laboratory Record Unknown Identifier #4 (All unknowns are nonelectrolytes, soi-1) Determination of the freezing point of pure l-butyl alcohol: (Record time-temperature data on the next page) 29.62 1. Mass of empty test tube 2. Mass of test tube and t-butyl alcohol after determination of freezing point of pure t-butyl alcohol 50.25 20.71 3. Mass of t-butyl alcohol Determination of the molar mass of an unknown: (Record time-temperature data...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass of benzoic acid grams) Freezing temperature of pure lauric acid (°C) From Part 8.02 11.04 g. 4 2.95 4 227900 Freezing point of the benzoic acid and lauricucid ("C) Part III: Unknown solute and lauric Acid Mass of lauric acid (grams) 8.0 49 Mass of unknown solute (grams) P.98g Freezing temperature of pure lauric acid ("C) (From Part 45°C Freezing point of the unknown...
1).A solute is a strong electrolyte that ionizes into 2 ions. What is the molar mass...
1).A solute is a strong electrolyte that ionizes into 2 ions. What is the molar mass of this solute if 22.34 grams added to exactly 1 kg of solvent change the boiling point by 0.871. (The Kb value for this solute is 0.577 °C/m). Record your answer as a whole number. 2). A sodium hydroxide solution that contains 15 grams of NaOH per L of solution has a density of 1.13 g/mL. Calculate the molality of the NaOH in this...
Hi, I need some help with Chemistry. Q1: Q2: Here is some background for the questions: Thank y...
Hi, I need some help with Chemistry.
Q1:
Q2:
Here is some background for the questions:
Thank you in advance.
You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...
Calculate the molar mass of the unknown acid A student knows or gathered the following information:...
Calculate the molar mass of the unknown acid A student knows or gathered the following information: Kf = 5.12 °C/m Tf (pure) = 35.7 °C Tf (solution) = 44.4 °C mass of solvent = 5.007 g mass of unknown acid = 1.006 g ΔTf = m * Kf Answer:________?
1.The freezing point of benzene is 5.5 °C. What is the molar mass of a nonionizing...
1.The freezing point of benzene is 5.5 °C. What is the molar mass of a nonionizing solute if 1.99 grams of the solute added to 20.62 g of benzene lowers the freezing point to 3.44. The Kf of benzene is -5.12 °C/m. Record your answer as a whole number. 2.Water has a Kf of -1.86 °C/m. Calculate the new freezing point of an aqueous solution made by mixing 38.66 g water and 1.64 g MgCl2. 3.Ethanol has a Kb of...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
Chemistry:
Molar mass determination and freezing point depression.
If your unknown solute sample weighed 0.634 grams, but some of it stuck to the test tube wall when you were pouring it in and did not dissolve in the t-butyl alcohol, what sort of error will this cause in the calculated molar mass of your unknown solute? Explain. What would be the freezing point of an aqueous solution that contains 10.3 grams of ethylene glycol [(C_2H_4(OH)_2] in 100 mL of water?
Freezing Point Depression: Determination of the Molar Mass of an Unknown Substance Laboratory Record Unknown Identifier #4 (All unknowns are nonelectrolytes, soi-1) Determination of the freezing point of pure l-butyl alcohol: (Record time-temperature data on the next page) 29.62 1. Mass of empty test tube 2. Mass of test tube and t-butyl alcohol after determination of freezing point of pure t-butyl alcohol 50.25 20.71 3. Mass of t-butyl alcohol Determination of the molar mass of an unknown: (Record time-temperature data...
A TARLES ca Part I: Benzoic acid and laurie Acid Mass of uric acid grams) Mass of benzoic acid grams) Freezing temperature of pure lauric acid (°C) From Part 8.02 11.04 g. 4 2.95 4 227900 Freezing point of the benzoic acid and lauricucid ("C) Part III: Unknown solute and lauric Acid Mass of lauric acid (grams) 8.0 49 Mass of unknown solute (grams) P.98g Freezing temperature of pure lauric acid ("C) (From Part 45°C Freezing point of the unknown...
Hi, I need some help with Chemistry.
Q1:
Q2:
Here is some background for the questions:
Thank you in advance.
You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...
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