Show one sample calculation to convert from % mass to molality. This is a ethylene glycol...
Show one sample calculation to convert from % mass to molality.
This is a ethylene glycol solution.
Mass % Ethylene glycol= 2.00, molality=0.32
mass %: 2= (0.50/25.01)x100
molality: 0.32=(0.50 x (1/62.06)) / ((25.01-0.50) x 1/1000)
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Show one sample calculation to convert from % mass to
molality.
This is a ethylene glycol...
Show one sample calculation to find the Tf for a 52.0% mass solution (again, use the...
Show one sample calculation to find the Tf for a 52.0% mass solution (again, use the trendline from the molality graph). (Hint: convert 52.0% to correct units!) The equation is Tf=0.485(m)+-0.134 where Tf is freezing temperature and m is molality. I'm guessing you have to convert percent mass to molality but I don't know how to do that. EDIT: It is a Ethylene glycol solution, so molar mass is 62.06.
What is the molality of ethylene glycol, C2H4(OH)2, in a solution prepared from 2.22 × 103...
What is the molality of ethylene glycol, C2H4(OH)2, in a solution prepared from 2.22 × 103 g of ethylene glycol and 2.00 × 103 g of water?
15. What is the molality of a solution made from 1 gal of ethylene glycol (density...
15. What is the molality of a solution made from 1 gal of ethylene glycol (density 1.11 g/ml) and I gal of water (density 1.00 g/ml)? 4 pts 16. Determine the freezing point and boiling point for the aqueous solution in number 15 above. Water is the solvent. 4 pts
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of...
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of...
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of ethylene glycol with a density of 1.0087 g/mL. The freezing point depression constant for water (which you can assume is the solvent for all solutions) is K1.86°C kg/mol and the boiling point elevation constant is Kb the following: 0.512°C kg/mol. The density of neat water at 20.0°C is 0.9982 g/ml. Answer 1. What is the molarity of the solution? 2. What is the molality...
2. Calculate the concentrations of solutions 1-7 from the procedure step 2. Show one sample calculation....
2. Calculate the concentrations of solutions 1-7 from the procedure step 2. Show one sample calculation. Test Tube # Concentration (M) 2. Prepare one solution at a time by pipeting the following volumes into a small beaker for mixing, then transfer the solution to the appropriate test tube. Test Tube No. 0.150 M COCI, (m.) 2.00 4.00 5.00 6.00 7.00 8.00 10.00 Distilled H,O (mL) 8.00 6.00 5.00 4.00 3.00 2.00 0.00
i need help using the formula in the 3rd picture , to figure picture 2(the molar...
i need help using the formula in the 3rd picture , to figure
picture 2(the molar mass). I included needed information in picture
1
Pure TBA, T9 Ethylene Glycol/TBA Solution, T Calculation of Molar Mass of Ethylene Glycol Mass of ethylene glycol used (total amount in solution) .94 253 t Mass of TBA used Freezing point of pure TBA, T Freezing point of solution, T, oC oc oC Freezing point depression (total dgpression), 471 Total molal concentration m of ethylene...
26.)Show the calculation of the mass of NaNO3 needed to make 450 ml of a 0.356...
26.)Show the calculation of the mass of NaNO3 needed to make 450 ml of a 0.356 M solution. 25.)Show the calculation of the molarity of a solution made by dissolving 15.9 grams of Ca3(PO4)2 to make 350 ml of solution. 24.)Show the calculation of the molarity of a solution made by dissolving 12.6 grams of NaNO3 to make 200 ml of solution. 23.Show the calculation of the molality of a solution made by dissolving 15.9 grams of Ca3(PO4)2 in 400...
Calculation required for Q. 2: Calculation of mass of CaCO3 sample for analysis.
calculation required for Q. 2: Calculation of mass of CaCO3
sample for analysis.
solid calcium carbhotae samples, calcium bicarbonate, CalHCO), i abo prscn. 1. In some calciunm for its reaction with hydrochloric acid. (og) 2 Experimental Procedure, Part A.2a. Complete the calculation required to appear on the Report Sheet (here and Report Sheet). 3. a. Experimental Procedure, Part A.3b. Explain how a water-filled graduated cylinder is inverted in a pan of water. b. Experimental Procedure, Part A.4. What is the...
The molar mass of a compound expresses the ratio of mass to moles Part A molar...
The molar mass of a compound expresses the ratio of mass to moles Part A molar mass- _mass in gr tert-Butyl alcohol is a solvent with a Kf of 9.10 °C/m and a freezing point of 25.5 °C. When 0.807 g of an unknown colorless liquid was dissolved in 11.6 g of tert-butyl alcohol, the solution froze at 15.3°C number of moles This quantity can be determined experimentally by accurately measuring the mass of the sample and determining the corresponding...
15. What is the molality of a solution made from 1 gal of ethylene glycol (density 1.11 g/ml) and I gal of water (density 1.00 g/ml)? 4 pts 16. Determine the freezing point and boiling point for the aqueous solution in number 15 above. Water is the solvent. 4 pts
A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of ethylene glycol with a density of 1.0087 g/mL. The freezing point depression constant for water (which you can assume is the solvent for all solutions) is K1.86°C kg/mol and the boiling point elevation constant is Kb the following: 0.512°C kg/mol. The density of neat water at 20.0°C is 0.9982 g/ml. Answer 1. What is the molarity of the solution? 2. What is the molality...
2. Calculate the concentrations of solutions 1-7 from the procedure step 2. Show one sample calculation. Test Tube # Concentration (M) 2. Prepare one solution at a time by pipeting the following volumes into a small beaker for mixing, then transfer the solution to the appropriate test tube. Test Tube No. 0.150 M COCI, (m.) 2.00 4.00 5.00 6.00 7.00 8.00 10.00 Distilled H,O (mL) 8.00 6.00 5.00 4.00 3.00 2.00 0.00
i need help using the formula in the 3rd picture , to figure
picture 2(the molar mass). I included needed information in picture
1
Pure TBA, T9 Ethylene Glycol/TBA Solution, T Calculation of Molar Mass of Ethylene Glycol Mass of ethylene glycol used (total amount in solution) .94 253 t Mass of TBA used Freezing point of pure TBA, T Freezing point of solution, T, oC oc oC Freezing point depression (total dgpression), 471 Total molal concentration m of ethylene...
calculation required for Q. 2: Calculation of mass of CaCO3
sample for analysis.
solid calcium carbhotae samples, calcium bicarbonate, CalHCO), i abo prscn. 1. In some calciunm for its reaction with hydrochloric acid. (og) 2 Experimental Procedure, Part A.2a. Complete the calculation required to appear on the Report Sheet (here and Report Sheet). 3. a. Experimental Procedure, Part A.3b. Explain how a water-filled graduated cylinder is inverted in a pan of water. b. Experimental Procedure, Part A.4. What is the...
The molar mass of a compound expresses the ratio of mass to moles Part A molar mass- _mass in gr tert-Butyl alcohol is a solvent with a Kf of 9.10 °C/m and a freezing point of 25.5 °C. When 0.807 g of an unknown colorless liquid was dissolved in 11.6 g of tert-butyl alcohol, the solution froze at 15.3°C number of moles This quantity can be determined experimentally by accurately measuring the mass of the sample and determining the corresponding...
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