Question

which is more important in determining  a compounds melting point, its polarity or its formula weight?

 

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Question

Question

Question 2How does adding a nonvolatile solute to a solvent impact vapor

pressure?

It decreases the vapor pressure

It increases the vapor pressure

It has no effect on the vapor pressure

Question 3

Water cannot dissolve _______________ compounds.

nonpolar

polar

ionic

Question 4

In a can of soda, which of the following is the solvent

carbon dioxide

water

sugar

Question 5

Explain why covalent compounds are unable to create electrolytes.

Question 6

What is a solution equilibrium?

A solution in which the rate of dissolving equals the rate of recrystallizing

A solution that has not been stirred

A solution in which all of the solute is dissolved

Question 7

How a supersaturated solution is usually prepared?

adding a large excess of solute to solvent and stirring vigorously

making an exactly saturated solution and allowing solvent to evaporate

heating a saturated solution until all of the solute dissolves, then cooling back down

Question 8

 A solution that contains the maximum possible amount of dissolved solute is _____.

supersaturated

unsaturated

saturated

Question 9

A solution in which 50 g of KClO3 is dissolved in 100 g of water at 90°C is _____.

none of these

unsaturated

saturated

super-saturated

Question 10

What is the molality of a solution prepared by dissolving 317 g of CaCl2 into 2.50 kg of water?

0.127 m

1.14 m

3.21 m

Question 11

45.0 g of Ca(NO3)2 was used to form a 0.80 M solution. What is the volume of the solution?

340 L

210 L

.34 L

Question 12

How many moles are present in a 4.25 m aqueous solution prepared with 400. g of water?

5.88 mol

1.70 mol

2.35 mol

Question 13

2.0 L of a 1.5 M solution is diluted with water until the final volume is 6.0 L. The molarity of the solution is now _____.

0.50 M

2.0 M

1.0 M

Question 14

A solution is made by dissolving a NaCl in water. Compared to the pure water, the solution

has a lower normal boiling point.

has a higher freezing point.

has a higher normal boiling point.

Question 15

What is the boiling point of a solution of ethanol, C2H5OH, and sugar, C12H22O11, that contains 20.00 g of the sugar in 250.0 g of ethanol?

78.12 C

78.69 C

100.285 C

Question 16

A sugar water solution has a freezing point of – 0.23oC. What is the molal concentration of the solution?

0.124 molal

0.101 molal

0.142 molal

Question 17

What is the freezing point of a solution in which 2.50 grams of sodium chloride is added to 230.0 mL of water?

Question 18

FOR FULL CREDIT BE SURE TO SHOW YOUR WORK.

What volume of a .20 M H3PO4 is needed to react with 100 mL of .1 M NaOH? 

H3PO4 + 3 NaOH –> Na3PO4 + 3 H2O

Question 2How does adding a nonvolatile solute to a solvent impact vapor

pressure?

It decreases the vapor pressure

It increases the vapor pressure

It has no effect on the vapor pressure

Question 3

Water cannot dissolve _______________ compounds.

nonpolar

polar

ionic

Question 4

In a can of soda, which of the following is the solvent

carbon dioxide

water

sugar

Question 5

Explain why covalent compounds are unable to create electrolytes.

Question 6

What is a solution equilibrium?

A solution in which the rate of dissolving equals the rate of recrystallizing

A solution that has not been stirred

A solution in which all of the solute is dissolved

Question 7

How a supersaturated solution is usually prepared?

adding a large excess of solute to solvent and stirring vigorously

making an exactly saturated solution and allowing solvent to evaporate

heating a saturated solution until all of the solute dissolves, then cooling back down

Question 8

 A solution that contains the maximum possible amount of dissolved solute is _____.

supersaturated

unsaturated

saturated

Question 9

A solution in which 50 g of KClO3 is dissolved in 100 g of water at 90°C is _____.

none of these

unsaturated

saturated

super-saturated

Question 10

What is the molality of a solution prepared by dissolving 317 g of CaCl2 into 2.50 kg of water?

0.127 m

1.14 m

3.21 m

Question 11

45.0 g of Ca(NO3)2 was used to form a 0.80 M solution. What is the volume of the solution?

340 L

210 L

.34 L

Question 12

How many moles are present in a 4.25 m aqueous solution prepared with 400. g of water?

5.88 mol

1.70 mol

2.35 mol

Question 13

2.0 L of a 1.5 M solution is diluted with water until the final volume is 6.0 L. The molarity of the solution is now _____.

0.50 M

2.0 M

1.0 M

Question 14

A solution is made by dissolving a NaCl in water. Compared to the pure water, the solution

has a lower normal boiling point.

has a higher freezing point.

has a higher normal boiling point.

Question 15

What is the boiling point of a solution of ethanol, C2H5OH, and sugar, C12H22O11, that contains 20.00 g of the sugar in 250.0 g of ethanol?

78.12 C

78.69 C

100.285 C

Question 16

A sugar water solution has a freezing point of – 0.23oC. What is the molal concentration of the solution?

0.124 molal

0.101 molal

0.142 molal

Question 17

What is the freezing point of a solution in which 2.50 grams of sodium chloride is added to 230.0 mL of water?

Question 18

FOR FULL CREDIT BE SURE TO SHOW YOUR WORK.

What volume of a .20 M H3PO4 is needed to react with 100 mL of .1 M NaOH? 

H3PO4 + 3 NaOH –> Na3PO4 + 3 H2O

 

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