What volume of a 0.771 M solution of CaCl2 contains 1.28 g of solute?

A) 66.8 mL B) 15.0 mL C) 1.66 mL D) 8.89 mL E) 85.0 mL A) 66.8 mL B) 15.0 mL C) 1.66 mL D) 8.89 mL E) 85.0 mL

A solution consisting of 0.228 mol of methylbenzene,C6H5CH3,in 255 g of nitrobenzene,C6H5NO2,freezes at -0.3°C.Pure nitrobenzene freezes at 6.0°C.What is the freezing-point depression constant of nitrobenzene?

A) 1.1°C/m B) 27°C/m C) 14.0°C/m D) 3.5°C/m E) 7.0°C/m A) 1.1°C/m B) 27°C/m C) 14.0°C/m D) 3.5°C/m E) 7.0°C/m

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

A) 0.000866 B) 0.0569 C) 0.271 D) 37.2 E) 59.2 A) 0.000866 B) 0.0569 C) 0.271 D) 37.2 E) 59.2

What concentration of silver nitrate (in ppm)is present in 7.1 $\times$ 10-7 M AgNO3(aq)? For very dilute aqueous solutions,you can assume the solution's density is 1.0 g/mL.The molar mass of AgNO3 is 169.9 g/mol.

A) 0.0071 ppm B) 0.12 ppm C) 0.71 ppm D) 1.7 ppm E) 8.3 ppm A) 0.0071 ppm B) 0.12 ppm C) 0.71 ppm D) 1.7 ppm E) 8.3 ppm

Which of the following statements concerning solubility is/are CORRECT? 1)Ionic compounds composed of Group 1A metal ions and halide ions,such as NaCl,are insoluble in nonpolar solvents. 2)The solubility of the halogens (Cl2,Br2,and I2)in polar solvents is greater than their solubility in nonpolar solvents. 3)The solubility of polar molecules,such as sugar,in polar solvents is generally greater than their solubility in nonpolar solvents.

A) 1 only B) 2 only C) 3 only D) 1 and 3 E) 1,2,and 3 A) 1 only B) 2 only C) 3 only D) 1 and 3 E) 1,2,and 3

If 11.2 g of naphthalene,C10H8,is dissolved in 105.4 g of chloroform,CHCl3,what is the molality of the solution?

A) 0.0875 m B) 12.7 m C) 0.830 m D) 0.0961 m E) 0.0991 m A) 0.0875 m B) 12.7 m C) 0.830 m D) 0.0961 m E) 0.0991 m

What is the molality of ethanol,C2H5OH,in an aqueous solution that is 37.4% ethanol by mass?

A) 0.597 m B) 0.0130 m C) 13.0 m D) 0.719 m E) 93.0 m A) 0.597 m B) 0.0130 m C) 13.0 m D) 0.719 m E) 93.0 m

Exam 14: Solutions and Their Behavior

What is the freezing point of a solution containing 2.80 grams benzene (molar mass = 78.11 g/mol)dissolved in 43.0 grams paradichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure paradichlorobenzene is 53.0 ^$\circ$C and the freezing point depression constant,K_fp,is -7.10 ^$\circ$C/m.

(Multiple Choice)

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Question 41

A surfactant used for cleaning is called a(n)________.

(Short Answer)

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Question 42

What is the mass of H₂SO₄ in a 46.4-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H₂SO₄?

(Multiple Choice)

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Question 43

Assuming ideal behavior,which of the following aqueous solutions would be expected to exhibit the $\underline{\text{ smallest}}$ freezing-point lowering?

(Multiple Choice)

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Question 44

A concentrated sodium hydroxide solution is 50.5% NaOH by mass and has a density of 1.53 g/mL at 25°C.What is the molarity of NaOH?

(Multiple Choice)

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Question 45

What volume of a 0.771 M solution of CaCl₂ contains 1.28 g of solute?

(Multiple Choice)

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Question 46

A solution consisting of 0.228 mol of methylbenzene,C₆H₅CH₃,in 255 g of nitrobenzene,C₆H₅NO₂,freezes at -0.3°C.Pure nitrobenzene freezes at 6.0°C.What is the freezing-point depression constant of nitrobenzene?

(Multiple Choice)

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Question 47

A solution in which there is more dissolved solute than in a saturated solution is known as a(n)________ solution.

(Short Answer)

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Question 48

What is the mole fraction of calcium chloride in 3.35 m CaCl₂(aq)? The molar mass of CaCl₂ is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

(Multiple Choice)

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Question 49

What concentration of silver nitrate (in ppm)is present in 7.1 $\times$ 10^-7 M AgNO₃(aq)? For very dilute aqueous solutions,you can assume the solution's density is 1.0 g/mL.The molar mass of AgNO₃ is 169.9 g/mol.

(Multiple Choice)

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Question 50

The standard enthalpy of formation of RbF(s)is -557.7kJ/mol and the standard enthalpy of formation of RbF(aq,1 m)is -583.8 kJ/mol.Determine the enthalpy of solution of RbF and indicate whether the solution temperature will increase or decrease when RbF is dissolved in water.

(Multiple Choice)

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Question 51

Which of the following statements concerning solubility is/are CORRECT? 1)Ionic compounds composed of Group 1A metal ions and halide ions,such as NaCl,are insoluble in nonpolar solvents. 2)The solubility of the halogens (Cl₂,Br₂,and I₂)in polar solvents is greater than their solubility in nonpolar solvents. 3)The solubility of polar molecules,such as sugar,in polar solvents is generally greater than their solubility in nonpolar solvents.

(Multiple Choice)

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Question 52

If one of the factors determining the equilibrium of a system is changed,the system adjusts to counteract that change.This is known as ________ principle.

(Short Answer)

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Question 53

A 0.20 M solution of MgSO₄ has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

(Multiple Choice)

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Question 54

If 11.2 g of naphthalene,C₁₀H₈,is dissolved in 105.4 g of chloroform,CHCl₃,what is the molality of the solution?

(Multiple Choice)

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Question 55

All of the following are colloidal dispersions EXCEPT ____.

(Multiple Choice)

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Question 56

Which of the following statements is/are CORRECT? 1)Solubility is defined as the concentration of solute in equilibrium with undissolved solute in a saturated solution. 2)If two liquids mix to an appreciable extent to form a solution,they are miscible. 3)If two liquids mix completely in any proportion to form a solution,the resulting solution is supersaturated.

(Multiple Choice)

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Question 57

What is the freezing point of an aqueous 1.36 m NaCl solution? (K_fp for water is 1.858°C/m.)Assume no ion pairing occurs.

(Multiple Choice)

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Question 58

What is the molality of ethanol,C₂H₅OH,in an aqueous solution that is 37.4% ethanol by mass?

(Multiple Choice)

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Question 59

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution.The osmotic pressure of the solution is 1.21 atm at 27 ^$\circ$C.What is the molar mass of the solute? (R = 0.08206 L.atm/mol.K)

(Multiple Choice)

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Question 60

Showing 41 - 60 of 83

Exam 14: Solutions and Their Behavior

A surfactant used for cleaning is called a(n)________.

What is the mass of H2SO4 in a 46.4-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H2SO4?

Assuming ideal behavior,which of the following aqueous solutions would be expected to exhibit the smallest‾\underline{\text{ smallest}} smallest​ freezing-point lowering?

A concentrated sodium hydroxide solution is 50.5% NaOH by mass and has a density of 1.53 g/mL at 25°C.What is the molarity of NaOH?

What volume of a 0.771 M solution of CaCl2 contains 1.28 g of solute?

A solution consisting of 0.228 mol of methylbenzene,C6H5CH3,in 255 g of nitrobenzene,C6H5NO2,freezes at -0.3°C.Pure nitrobenzene freezes at 6.0°C.What is the freezing-point depression constant of nitrobenzene?

A solution in which there is more dissolved solute than in a saturated solution is known as a(n)________ solution.

What is the mole fraction of calcium chloride in 3.35 m CaCl2(aq)? The molar mass of CaCl2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

What concentration of silver nitrate (in ppm)is present in 7.1 ×\times× 10-7 M AgNO3(aq)? For very dilute aqueous solutions,you can assume the solution's density is 1.0 g/mL.The molar mass of AgNO3 is 169.9 g/mol.

The standard enthalpy of formation of RbF(s)is -557.7kJ/mol and the standard enthalpy of formation of RbF(aq,1 m)is -583.8 kJ/mol.Determine the enthalpy of solution of RbF and indicate whether the solution temperature will increase or decrease when RbF is dissolved in water.

If one of the factors determining the equilibrium of a system is changed,the system adjusts to counteract that change.This is known as ________ principle.

A 0.20 M solution of MgSO4 has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

If 11.2 g of naphthalene,C10H8,is dissolved in 105.4 g of chloroform,CHCl3,what is the molality of the solution?

All of the following are colloidal dispersions EXCEPT ____.

What is the freezing point of an aqueous 1.36 m NaCl solution? (Kfp for water is 1.858°C/m.)Assume no ion pairing occurs.

What is the molality of ethanol,C2H5OH,in an aqueous solution that is 37.4% ethanol by mass?

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution.The osmotic pressure of the solution is 1.21 atm at 27 ∘\circ∘ C.What is the molar mass of the solute? (R = 0.08206 L.atm/mol.K)

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What is the mass of H₂SO₄ in a 46.4-mL sample of concentrated sulfuric acid that has a density of 1.84 g/mL and consists of 98.3% H₂SO₄?

Assuming ideal behavior,which of the following aqueous solutions would be expected to exhibit the $\underline{\text{ smallest}}$ freezing-point lowering?

What volume of a 0.771 M solution of CaCl₂ contains 1.28 g of solute?

A solution consisting of 0.228 mol of methylbenzene,C₆H₅CH₃,in 255 g of nitrobenzene,C₆H₅NO₂,freezes at -0.3°C.Pure nitrobenzene freezes at 6.0°C.What is the freezing-point depression constant of nitrobenzene?

What is the mole fraction of calcium chloride in 3.35 m CaCl₂(aq)? The molar mass of CaCl₂ is 111.0 g/mol and the molar mass of water is 18.02 g/mol.

What concentration of silver nitrate (in ppm)is present in 7.1 $\times$ 10^-7 M AgNO₃(aq)? For very dilute aqueous solutions,you can assume the solution's density is 1.0 g/mL.The molar mass of AgNO₃ is 169.9 g/mol.

A 0.20 M solution of MgSO₄ has an observed osmotic pressure of 7.7 atm at 25°C.Determine the observed van't Hoff factor for this experiment.

If 11.2 g of naphthalene,C₁₀H₈,is dissolved in 105.4 g of chloroform,CHCl₃,what is the molality of the solution?

What is the freezing point of an aqueous 1.36 m NaCl solution? (K_fp for water is 1.858°C/m.)Assume no ion pairing occurs.

What is the molality of ethanol,C₂H₅OH,in an aqueous solution that is 37.4% ethanol by mass?

A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution.The osmotic pressure of the solution is 1.21 atm at 27 ^$\circ$C.What is the molar mass of the solute? (R = 0.08206 L.atm/mol.K)