## General Chemistry

##
Chemistry of Solutions Flashcard List

**10**flashcards

Loading....

×

Coupon Accepted Successfully!
×

Open Flashcards

Get access to all chapters

Question

Equivalents of solute per liter of solution is:

A | Molality |

B | Molarity |

C | Normality |

D | None of the above |

Flip

Question

The concentration of a given solution of glucose (C

A | 1.5 M |

B | 0.67 M |

C | 4.86 M |

D | 270 M |

Flip

Question

You are presented with a 2.5

A | 36.5 g |

B | 91.25 g |

C | 111 g |

D | 114 g |

Flip

Question

You are asked to prepare 30 ml of a 2

A | 3 ml |

B | 6 ml |

C | 10 ml |

D | 30 ml |

Flip

Question

How many grams of NaCl are required to prepare 250 ml of 0.35

A | 0.0875 g |

B | 20.5 g |

C | 5.1 g |

D | 87.5 g |

Flip

Question

The concentration of solutions are generally expressed in terms of molarity, molality, normality, and weight percent. The formation of the solutions itself has many ramifications. The solubility of solutes differ considerably from one other. Some of the factors that can influence the solubility include temperature and pressure. Solubility depends on other factors as well. Given below in Figure-1 is a graph which depicts solubility differences of some solutes.

Quite often, the freezing and boiling point changes that are brought about by the dissolved solutes can be predicted reasonably. But this is not always the case.

The predictions and calculations are done for freezing point depression (ΔT_{f}) based on the following formula:

ΔT_{f} = K_{f} m,

where m is the molality and K_{f} is the freezing point depression constant. (K_{f}= 1.86 ^{o}C/*m*)

For boiling point elevation (ΔT_{b}), the calculations are based on the following formula:

ΔT_{b} = K_{b} m,

where m is the molality and K_{b} is the boiling point elevation constant. (K_{b} = 0.512 ^{o}C/*m*)

The graph in the passage shows the solubilities of some compounds (salts). Which of the following is most likely true regarding the Compounds A, B, C and D?

A | The solubility process of Compound B is exothermic, and those of Compounds A, C and D are endothermic |

B | The solubility process of Compound B is endothermic, and those of Compounds A, C and D are exothermic |

C | The solubility processes of Compounds A, B, C and D are exothermic |

D | The solubility processes of Compounds A, B, C and D are endothermic |

Flip

Question

The concentration of solutions are generally expressed in terms of molarity, molality, normality, and weight percent. The formation of the solutions itself has many ramifications. The solubility of solutes differ considerably from one other. Some of the factors that can influence the solubility include temperature and pressure. Solubility depends on other factors as well. Given below in Figure-1 is a graph which depicts solubility differences of some solutes.

Quite often, the freezing and boiling point changes that are brought about by the dissolved solutes can be predicted reasonably. But this is not always the case.

The predictions and calculations are done for freezing point depression (ΔT_{f}) based on the following formula:

ΔT_{f} = K_{f} m,

where m is the molality and K_{f} is the freezing point depression constant. (K_{f}= 1.86 ^{o}C/*m*)

For boiling point elevation (ΔT_{b}), the calculations are based on the following formula:

ΔT_{b} = K_{b} m,

where m is the molality and K_{b} is the boiling point elevation constant. (K_{b} = 0.512 ^{o}C/*m*)

A solution was made by using 315 g of glucose in 750 g of water. What is the boiling point of this solution?

A | 98.8^{0} C |

B | 99.8^{0} C |

C | 100.24^{0} C |

D | 101.2^{0} C |

Flip

Question

The concentration of solutions are generally expressed in terms of molarity, molality, normality, and weight percent. The formation of the solutions itself has many ramifications. The solubility of solutes differ considerably from one other. Some of the factors that can influence the solubility include temperature and pressure. Solubility depends on other factors as well. Given below in Figure-1 is a graph which depicts solubility differences of some solutes.

Quite often, the freezing and boiling point changes that are brought about by the dissolved solutes can be predicted reasonably. But this is not always the case.

The predictions and calculations are done for freezing point depression (ΔT_{f}) based on the following formula:

ΔT_{f} = K_{f} m,

where m is the molality and K_{f} is the freezing point depression constant. (K_{f}= 1.86 ^{o}C/*m*)

For boiling point elevation (ΔT_{b}), the calculations are based on the following formula:

ΔT_{b} = K_{b} m,

where m is the molality and K_{b} is the boiling point elevation constant. (K_{b} = 0.512 ^{o}C/*m*)

Two experiments were conducted for analyzing the solubility properties and their effects on colligative properties. In Experiment I, a 1.0 *m* solution of KBr was analyzed and in Experiment II, a 2.3 *m* solution of KBr was analyzed. The experimental values of freezing and boiling points were slightly different from the expected values based on the theoretical calculations discussed in the passage. Which of the following is most likely correct regarding the two experiments?

A | The experimental values of the solution in Experiment I was more different from the theoretical calculations than the solution in Experiment II |

B | The experimental values of the solution in Experiment II was more different from the theoretical calculations than the solution in Experiment I |

C | Both experiments have the same extent of differences from the theoretical predictions |

D | The discrepancy noted in the experiments is absolutely a result of instrumental error, because the differences in Experiments I & II cannot change colligative properties |

Flip

Question

_{f}) based on the following formula:

ΔT_{f} = K_{f} m,

_{f} is the freezing point depression constant. (K_{f}= 1.86 ^{o}C/*m*)

For boiling point elevation (ΔT_{b}), the calculations are based on the following formula:

ΔT_{b} = K_{b} m,

_{b} is the boiling point elevation constant. (K_{b} = 0.512 ^{o}C/*m*)

If the amount of glucose used in Question 7 is doubled, while the same 750 g of water was used, what must have happened to the boiling point of the solution?

A | It doubled |

B | It quadrupled |

C | It decreased slightly |

D | It increased slightly |

Flip

Question

_{f}) based on the following formula:

ΔT_{f} = K_{f} m,

_{f} is the freezing point depression constant. (K_{f}= 1.86 ^{o}C/*m*)

For boiling point elevation (ΔT_{b}), the calculations are based on the following formula:

ΔT_{b} = K_{b} m,

_{b} is the boiling point elevation constant. (K_{b} = 0.512 ^{o}C/*m*)

Which of the following statements is true regarding solutions?

A | As the concentration of a solution increases, the vapor pressure increases |

B | As the concentration of a solution decreases, the vapor pressure decreases |

C | As the concentration of a solution increases, the vapor pressure decreases |

D | None of the above |

Flip