14. Solutions

Determine the Mole Fraction in 1.00 L of 2.20 M NaCl

Determine the Mole Fraction in 1.00 L of 2.20 M NaCl

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chemistNATE

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How to calculate the mole fraction of a component is a solution?

$How to calculate the mole fraction of a component is a solution?$

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Dr. V

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Practice this topic

Multiple Choice

Calculate mole fraction of a 2.4 m aqueous solution of citric acid (C₆H₈O₇).

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Multiple Choice

If mole fraction of urea is 4.55 x 10^-1, what is the mass of urea needed to dissolve in 38.0 g of water? The molar mass of urea is 60.062 g/mol.

Calculate the mole fraction of sucrose (molar mass = 342.3 g/mol) in an aqueous solution that is 1.80 M sucrose? The density of solution is 1.08 g/mL.

Multiple Choice

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The density of acetonitrile 1CH3CN2 is 0.786 g>mL and the density of methanol 1CH3OH2 is 0.791 g>mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (a) What is the mole fraction of methanol in the solution?

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The density of toluene 1C7H82 is 0.867 g>mL, and the density of thiophene 1C4H4S2 is 1.065 g>mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole fraction of thiophene in the solution.

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Caffeine 1C8H10N4O22 is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform 1CHCl32 has a concentration of 0.0500 m, calculate (b) the mole fraction of caffeine in the solution.

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How would you prepare each of the following solutions? (c) A solution of methyl alcohol (methanol) and water in which Xmethanol = 0.15 and Xwater = 0.85

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A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g>mL and 1.00 g>mL, respectively. For this solution, calculate the concentration in each unit. e. mole percent

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An aqueous solution contains 36% HCl by mass. Calculate the molality and mole fraction of the solution.

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What is the concentration of each of the following solutions? (b) The mole fraction of each component of a solution pre- pared by dissolving 2.25 g of nicotine, C10H14N2, in 80.0 g of CH2Cl2

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Household bleach is a 5.0 mass % aqueous solution of sodium hypochlorite, NaOCl. What is the molality of the bleach? What is the mole fraction of NaOCl in the bleach?

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A 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20 °C. What is the concentration of this solution in the following units?(a) Mole fraction

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The estimated average concentration of NO2 in air in the United States in 2006 was 0.016 ppm. (a) Calculate the partial pressure of the NO2 in a sample of this air when the atmospheric pressure is 755 torr (99.1 kPa).

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Lactose, C12H22O11, is a naturally occurring sugar found in mammalian milk. A 0.335 M solution of lactose in water has a density of 1.0432 g/L at 20 °C. What is the concentra- tion of this solution in the following units? (b) Mass percent

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Acetonitrile 1CH3CN2 is a polar organic solvent that dissolves a wide range of solutes, including many salts. The density of a 1.80 M LiBr solution in acetonitrile is 0.826 g>cm3. Calculate the concentration of the solution (b) mole fraction of LiBr,

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Find the mass of urea (CH4N2O) needed to prepare 50.0 g of a solution in water in which the mole fraction of urea is 0.0770.

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Open Question

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

Open Question

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁) in 495 g of water. Determine the mole fraction of sucrose if the final volume of the solution is 508 ml.

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