How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution

A) 769 g B) 36.2 g C) 100. g D) 0.157 g E) 157 g A) 769 g B) 36.2 g C) 100. g D) 0.157 g E) 157 g

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq) solution that has a density of 1.015 g/mL

A) 2.09 % B) 2.29 % C) 2.49 % D) 2.69 % E) None of the above A) 2.09 % B) 2.29 % C) 2.49 % D) 2.69 % E) None of the above

Exam 12: Physical Properties of Solutions

The concentration of nitrogen in water at 25^$\circ$C was determined to be 7.2 * 10^-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25^$\circ$C is 6.8 * 10^-4 mol/L·atm.

(Multiple Choice)

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Question 61

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane. Hexane is the solute.

(True/False)

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Question 62

An endothermic solution process is described by which of the following

(Multiple Choice)

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Question 63

How many grams of propanol (C₃H₇OH, 60.10 g/mol) would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25^$\circ$C (R = 0.0821 L·atm/K·mol)

(Multiple Choice)

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Question 64

To interconvert the concentration units of molarity (M) and mass percent, you must also know the density of the solution.

(True/False)

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Question 65

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

(Multiple Choice)

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Question 66

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true

(Multiple Choice)

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Question 67

What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 g/mL

(Multiple Choice)

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Question 68

According to Raoult's law, which statement is false

(Multiple Choice)

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Question 69

What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 100. g of benzene by 0.47^$\circ$C K_f of benzene is 5.12^$\circ$C/m.

(Multiple Choice)

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Question 70

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution

(Multiple Choice)

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Question 71

For water K_f = 1.86^$\circ$C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol) solutions are the same.

(True/False)

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Question 72

Which of the following aqueous solutions has the highest boiling point (assume 100% dissociation for all soluble ionic compounds)

(Multiple Choice)

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Question 73

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25^$\circ$C K_b of water is 0.52^$\circ$C/m. Assume the density of the solution is the same as that of pure water.

(Multiple Choice)

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Question 74

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq) solution that has a density of 1.015 g/mL

(Multiple Choice)

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Question 75

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25^$\circ$C. Find the temperature at which this solution freezes. [Given: for water K_f = 1.86 ^$\circ$C/m; molecular mass of fructose = 180.16 g/mol]

(Multiple Choice)

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Question 76

Oxygen gas makes up 21 % of the atmosphere by volume. What is the solubility of O₂(g) in water at 25^$\circ$C if the atmospheric pressure is 741 mmHg The Henry's law constant for oxygen gas at 25^$\circ$C is 1.3 * 10^-3 mol/L·atm.

(Multiple Choice)

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Question 77

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5^$\circ$C For water K_f = 1.86^$\circ$C/m and K_b = 0.52^$\circ$C/m.

(Multiple Choice)

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Question 78

Calculate the mole fraction of KI in a solution made by dissolving 3.4 g of KI in 5.8 g of water.

(Multiple Choice)

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Question 79

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i

(Multiple Choice)

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Question 80

Showing 61 - 80 of 122

Exam 12: Physical Properties of Solutions

The concentration of nitrogen in water at 25 ∘\circ∘ C was determined to be 7.2 * 10-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25 ∘\circ∘ C is 6.8 * 10-4 mol/L·atm.

A solution made of pentane and hexane has a mole fraction, X = 0.250 of pentane. Hexane is the solute.

An endothermic solution process is described by which of the following

How many grams of propanol (C3H7OH, 60.10 g/mol) would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25 ∘\circ∘ C (R = 0.0821 L·atm/K·mol)

To interconvert the concentration units of molarity (M) and mass percent, you must also know the density of the solution.

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Consider a solution made from a nonvolatile solute and a volatile solvent. Which statement is true

What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 g/mL

According to Raoult's law, which statement is false

What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 100. g of benzene by 0.47 ∘\circ∘ C Kf of benzene is 5.12 ∘\circ∘ C/m.

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution

For water Kf = 1.86 ∘\circ∘ C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol) solutions are the same.

Which of the following aqueous solutions has the highest boiling point (assume 100% dissociation for all soluble ionic compounds)

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25 ∘\circ∘ C Kb of water is 0.52 ∘\circ∘ C/m. Assume the density of the solution is the same as that of pure water.

What is the percent by mass of sodium phosphate in a 0.142 M Na3PO4(aq) solution that has a density of 1.015 g/mL

An aqueous fructose solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25 ∘\circ∘ C. Find the temperature at which this solution freezes. [Given: for water Kf = 1.86 ∘\circ∘ C/m; molecular mass of fructose = 180.16 g/mol]

Oxygen gas makes up 21 % of the atmosphere by volume. What is the solubility of O2(g) in water at 25 ∘\circ∘ C if the atmospheric pressure is 741 mmHg The Henry's law constant for oxygen gas at 25 ∘\circ∘ C is 1.3 * 10-3 mol/L·atm.

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5 ∘\circ∘ C For water Kf = 1.86 ∘\circ∘ C/m and Kb = 0.52 ∘\circ∘ C/m.

Calculate the mole fraction of KI in a solution made by dissolving 3.4 g of KI in 5.8 g of water.

Assuming 100% dissociation, which of the following compounds is listed correctly with its van't Hoff factor i

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The concentration of nitrogen in water at 25^$\circ$C was determined to be 7.2 * 10^-6 M. Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25^$\circ$C is 6.8 * 10^-4 mol/L·atm.

How many grams of propanol (C₃H₇OH, 60.10 g/mol) would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25^$\circ$C (R = 0.0821 L·atm/K·mol)

What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 100. g of benzene by 0.47^$\circ$C K_f of benzene is 5.12^$\circ$C/m.

How many grams of water are needed to dissolve 27.8 g of ammonium nitrate NH₄NO₃ in order to prepare a 0.452 m solution

For water K_f = 1.86^$\circ$C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol) solutions are the same.

What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25^$\circ$C K_b of water is 0.52^$\circ$C/m. Assume the density of the solution is the same as that of pure water.

What is the percent by mass of sodium phosphate in a 0.142 M Na₃PO₄(aq) solution that has a density of 1.015 g/mL

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25^$\circ$C. Find the temperature at which this solution freezes. [Given: for water K_f = 1.86 ^$\circ$C/m; molecular mass of fructose = 180.16 g/mol]

Oxygen gas makes up 21 % of the atmosphere by volume. What is the solubility of O₂(g) in water at 25^$\circ$C if the atmospheric pressure is 741 mmHg The Henry's law constant for oxygen gas at 25^$\circ$C is 1.3 * 10^-3 mol/L·atm.

What is the freezing point of an aqueous solution of a nonvolatile solute that has a boiling point of 102.5^$\circ$C For water K_f = 1.86^$\circ$C/m and K_b = 0.52^$\circ$C/m.