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2. If 100. of liquid water 100.°C and 200. grams of water at 20.0°C are mixed...
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved...
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by...
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by 0.821°C. What is the Van't Hoff factor for this electrolyte? The freezing point depression constant for water is 1.86 °C/m. a. 0.521 b. 1.92 c. 2.00 d. 2.30 e. 4.41
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporizati...
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporization of water = 2.4 kJ/g) (specific heat of water = 4.18J/mole K) A) 1.6 x 10 g B) 2.3 x 103g C) 2.6 g D) 1.6 g E) 2.3 g
.stonl sample of a 60 M solution of HCI is diluted to 200, mL A) 240...
.stonl sample of a 60 M solution of HCI is diluted to 200, mL A) 240 M 8) 6.0 M WI 2.10M D) 1.50 M E) 2.00 M 21) 21) Which one of the following would act like a strong electrolyte in an aqueous solution? A) NH3 B) CH3OH C) CCl4 22) 22) In which of the following pairs of ionic compounds are both chemical species soluble in water? A) Be(NO312 and Bes(PO4)2 C)Cu S and PbBr2 B) NH4F and...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
QUESTION 31 A solution was made by dissolving 26.5g of Na2CO3 in 500.0 mL of water....
QUESTION 31 A solution was made by dissolving 26.5g of Na2CO3 in 500.0 mL of water. What is the molality of this solution? (1.0g of water -1.0 ml of water) 11 Na23.6C128016 OA 0.25 m OB. 0.25 M OC 0.5M OD 0.5 m E. None of above QUESTION 32 Molarity (M) of a solution varies with O A Pressure O Temperature OC Partial pressure D. Both A and B OE. Both A and C QUESTION 33 Which of the following...
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezin...
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C....
Pre-Laboratory Questions 1. The freezing point of 20.024 grams of distilled water was determined by recording...
Pre-Laboratory Questions 1. The freezing point of 20.024 grams of distilled water was determined by recording a thermogram (see plot below). 1.006 grams of an unknown, nonelectrolyte compound was added to the water, and a second thermogram was recorded to determine the freezing point of the solution. Freezing Point Curves for Water and Unknown Nonelectrolyte Temperature, c -Water -0.270 °C Time, s a. Determine the freezing point depression, Tg, for the unknown solution. b. Determine the molality, m, of the...
How much heat required to convert 36 grams (2 moles) of ice at 0 degrees C...
How much heat required to convert 36 grams (2 moles) of ice at 0 degrees C to liquid water at 50 degrees C? delta-H of fusion for H2O is 6.02 kJ/mol and the heat capacity of liquid water is 4.18J/g degrees C. A) 12 kJ B) 7524 J C) 8728 J D) 19564 J
Question 1. A 2.700×10−2M solution of NaCl in water is at 20.0∘C. The sample was created...
Question 1. A 2.700×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL. a.)Calculate the molality of the salt solution. B.) Calculate the mole fraction of salt in this solution. C.) Calculate the concentration of...
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by 0.821°C. What is the Van't Hoff factor for this electrolyte? The freezing point depression constant for water is 1.86 °C/m. a. 0.521 b. 1.92 c. 2.00 d. 2.30 e. 4.41
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporization of water = 2.4 kJ/g) (specific heat of water = 4.18J/mole K) A) 1.6 x 10 g B) 2.3 x 103g C) 2.6 g D) 1.6 g E) 2.3 g
.stonl sample of a 60 M solution of HCI is diluted to 200, mL A) 240 M 8) 6.0 M WI 2.10M D) 1.50 M E) 2.00 M 21) 21) Which one of the following would act like a strong electrolyte in an aqueous solution? A) NH3 B) CH3OH C) CCl4 22) 22) In which of the following pairs of ionic compounds are both chemical species soluble in water? A) Be(NO312 and Bes(PO4)2 C)Cu S and PbBr2 B) NH4F and...
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
QUESTION 31 A solution was made by dissolving 26.5g of Na2CO3 in 500.0 mL of water. What is the molality of this solution? (1.0g of water -1.0 ml of water) 11 Na23.6C128016 OA 0.25 m OB. 0.25 M OC 0.5M OD 0.5 m E. None of above QUESTION 32 Molarity (M) of a solution varies with O A Pressure O Temperature OC Partial pressure D. Both A and B OE. Both A and C QUESTION 33 Which of the following...
Pre-Laboratory Questions 1. The freezing point of 20.024 grams of distilled water was determined by recording a thermogram (see plot below). 1.006 grams of an unknown, nonelectrolyte compound was added to the water, and a second thermogram was recorded to determine the freezing point of the solution. Freezing Point Curves for Water and Unknown Nonelectrolyte Temperature, c -Water -0.270 °C Time, s a. Determine the freezing point depression, Tg, for the unknown solution. b. Determine the molality, m, of the...
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