(Solution) An aqueous potassium nitrate solution has a freezing point of -2.0 C. How many moles of potassium nitrate are contained in 0.5 kg of water in this > Snapessays.com

(Solution) An aqueous potassium nitrate solution has a freezing point of -2.0 C. How many moles of potassium nitrate are contained in 0.5 kg of water in this

An aqueous potassium nitrate solution has a freezing point of -2.0 ?C. How many moles of potassium nitrate are contained in 0.5 kg of water in this solution? The freezing point depression constant for water is -1.86 ?C/m.

(Points : 10)

0.21 moles

0.53 moles

1.2 moles

2.4 moles

2.

Concentrated NaOH is 12 M and has a density of 1.53 g/mL. What is the percent NaOH by mass of concentrated NaOH?

(Points : 10)

31.4%

49.5%

50.5%

73.8%

3.

What concentration unit is necessary for the calculation of boiling point elevation?

(Points : 10)

mole fraction of solute

mass fraction of solvent

molarity of solute

molality solute

4.

Which of the following pairs of liquids will be immiscible?

(Points : 10)

CCl4 and CH3H

H2O and C6H6

C6H14 and C8H18

C8H18 and oil

5.

What is the osmotic pressure of 0.1 M aqueous urea (CON2H4) at 30 ?C? (R = 0.08206 L•atm/mol•K)

(Points : 10)

0.51 atm

4.9 atm

6.1 atm

2.5 atm

6.

Which of the following statements concerning the solubility of a solute are correct?

1. The solubility of a gas in a liquid increases with increasing temperature.

2. The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

3. The dissolution of a gas in a liquid is an endothermic process.

(Points : 10)

1 only

2 only

3 only

2 and 3

7.

What is the molar mass of a nonelectrolyte if 6.02 grams dissolved in 30.0 grams of benzene freezes at -1.55 ?C? The freezing point of pure benzene is 5.50 ?C and the freezing point depression constant, Kfp, is -5.12 ?C/m.

(Points : 10)

146 g/mol

187 g/mol

276 g/mol

663 g/mol

8.

Predict which of the following compounds will have the lowest freezing point.

(Points : 10)

pure H2O

1 m NH3

1 m NaCl

1 m Ca(NO3)2

9.

What quantity of ethylene glycol, HOCH2CH2OH, must be added to 50 grams of water to raise the boiling point by 1.0 C? Express this answer in grams.

(Points : 10)

6.05 grams

4.35 grams

24.3 grams

23.7 grams

10.

What is the boiling point of a mixture composed of 85 g HOCH2CH2OH (ethylene glycol) and 125 g H2O? The boiling point elevation constant for H2O is 0.512 ?C/m.

(Points : 10)

100.2 ?C

105.6 ?C

107.1 ?C

135.2 ?C

11.

Sea water has a sodium (Na+) concentration of 1.08 x 104 ppm. If the solution is present as dissolved NaCl, what mass of NaCl is in each liter of sea water? Seawater has a density of 1.05 g/mL.

(Points : 10)

27.46 g

450 g

22.4 g

89 g

12.

A mass of 0.750 g calcium chloride is diluted with 975 g H2O. What is the chloride ion concentration (in ppm)?

(Points : 10)

81.8 ppm

164 ppm

251 ppm

492 ppm

13.

What is the molality of a solution prepared by dissolving 300 g KCl in 225 g H2O?

(Points : 10)

0.0880 m

17.9 m

0.773 m

1.29 m

14.

The vapor pressure of pure water at 50.0 ?C is 92.5 mm Hg. Calculate the ideal partial pressure of water at this temperature for a mixture of 45.0 g H2O and 55.0 g CH3OH?

(Points : 10)

41.6 mm Hg

45.2 mm Hg

50.9 mm Hg

54.8 mm Hg

15.

What is the equilibrium concentration of carbon dioxide in water that is in contact with air at 25 ?C and 0.982 atm. The mole fraction of CO2 in air is 3.01 ? 10-4. The Henry's law constant for carbon dioxide is 4.48 ? 10-5 M/mm Hg.

(Points : 10)

1.32 ? 10-8 M

1.01 ? 10-5 M

8.68 ? 10-3 M

3.34 ? 10-2 M

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