CHEM 100 Lecture Notes - Lecture 16: Sodium Chloride, Molar Concentration, Intermolecular Force

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4 Dec 2017

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Identify a solute/solvent; types: factors that affect solubility, degree of saturation b. Intermolecular forces s/l like dissolves like i. g molar mass: pressure, temperature, qualitative analysis, molarity, molality, % concentration, dilutions, colligative properties, vp depression (vapor point, freezing point depression, bp increases, os. pressure increases. Saturated solution: solution containing the maximum possible amount of dissolved solute at the equilibrium. Henry"s law solubility= kp (constant depends on gas) Can either dissolve or crystalize the solution. Unsaturated + solute dissolved until equilibrium. As temperature increases the solubility or a solid in the solvent also increases. Most gases become less soluble in water as temperature rises. Molarity (m)= moles of solute/ liters of solution. Calculate molarity 4. 75 mol nacl to produce 3. 00 l solution. 4. 75 mol nacl/ 3. 00 l = 1. 58 m. Molality (m)= moles of solute/mass of solvent (kg) Percent by volume = volume of solute/ volume of solution (x) 100%

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DETERMINATION oF MOLAR EXPERIMENT 23 MASS FROM FREEZING POINT DEPRESSION EQUIPMENT AND CHEMICALS: Equipment 600 mL beaker Chemicals Cyclohexane (C Stir plate 100 ml. graduated cylinder Clamp Nonvolatile Unknowns Freezing point apparatus Spin vane 0.1 C Thermometer INTRODUCTION: When a solute is introduced into a pure solvent the newly formed solution will have certain physical properties that are from the solvent. As a of the presence of the the pressure of the solution will be lower than that of the pure solvent. As the vapor pressure is lowered there is a resulting increase in the amount of energy required to reach the boiling point of the solution. Conversely, the solution must cool to a lower temperature before a state change from liquid to solid occurs. These changes in physical properties vapor pressure lowering, boiling point elevation and freezing point depression are collectively referred to as colligative properties. These colligative properties, which also include osmotic pressure, do not depend on the nature of the nonvolatile solute in the solution but rather on the concentration of solute present. Because the properties are independent of the nature of the solute, they may be used to determine other properties of the solute such as molecular weight. The effect of a nonvolatile, nonelectrolyte solute on a pure solvent will be examined by finding the freezing point depression of a cyclohexane unknown so solution. The freezing point of a pure sample of cyclohexane will be determined. Introducing a nonelectrolyte solute should in solution formed to freeze at a lower temperature. This temperature will then be experimentally determined As stated the The molality of the solution dependent on the quantity of solute particles present in solution. (moles solute particles per kilogram of solvent) is directly proportional to the change in temperature between the freezing point of the pure solvent and that of the ATfss Kim The molal freezing point depression constant, K for cyclohexane is equal to 20.00 cfmolal By experimentally determining the freezing point depression of a ohexanel unknown solution, the molal concentration is easily calculated. In turn the molar mass of the unknown olute can be calculated as well Chemistry 132 EXPERIMENT23

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- Which of the following properly describes a colligative property of a solution?
A) a solution property that depends on the identity of the solute particles present
B) a solution property that depends on the electrical charges of the solute particles present
C) a solution property that depends on the amount of solute particles present
D) a solution property that depends on the pressure of the solute particles present
E) a solution property that depends on the amount, identity, and pressure of the solute particles present

- Which statement best explains the meaning of the phrase "like dissolves like"?
A. The only true solutions are formed when water dissolves a polar solute.
B. The only true solutions are formed when water dissolves a non-polar solute.
C. A solvent and solute with similar intermolecular forces will readily form a solution. D. A solvent will easily dissolve a solute of similar mass.

E. None of these statements is correct.

- The solubility of gases in liquids
A. increases as temperature increases and decreases as pressure increases

B. increases as temperature increases and increases as pressure increases

C. is independent of temperature and increases as pressure increases
D. decreases as temperature increases and increases as pressure increases

E. decreases as temperature increases and decreases as pressure increases

CHEM 100 Lecture Notes - Lecture 16: Sodium Chloride, Molar Concentration, Intermolecular Force

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