When potassium chloride (KCl) is dissolved in water the temperature decreases. Fill in the blanks to explain why this occurs. The energy required to separate the K* and Cl and to separate the water molecules is v the energy produced by the attractions between the K+ and Cl. less than - greater than

An aqueous solution is prepared by dissolving 0.050 mole of formic acid, HCOOH, in 1.00 kg of water.  The solution begins to freeze at -0.0986˚C.   Calculate the van’t Hoff factor for formic acid.  Ignore sig figs; give the answer to 3 decimal spaces

Assuming ideal solution behavior, what is the boiling point (in °C) of a solution of LiF in water (K = 0.513°C/m; K₁ = 1.86°C/m) if the solution freezes at -0.79°C? 102.8 X °C

What molality of Na Clis required to lower the freezing point of water to -11.6 degrees C? Use 1.853 degrees C/m for Kf of water.

How many grams of NaCl is needed to add to 1.0 kg of H2O resulting in a solution where the freezing point is -8.3 degree C? The molar mass of NaCl is 58.44 g/mol. The Kf value of H2O is 1.86 C/m. Do NOT type in the unit (g). 130.4

Octane (C3H₁8) has a vapor pressure of 14.3 torr and a density of 0.703 g/mL. Benzene (CH) has a vapor pressure of 105.0 torr and a density of 0.876 g/mL. Calculate the vapor pressure (in torr) of a solution containing 655 mL of octane and 325 mL of benzene. Assume this solution behaves ideally. torr

Increase in the temperature during summer months increases solubility of oxygen in bodies of water. The increase of dissolved oxygen in warm water holds more of dissolved oxygen than cool or cold water. O true O false

Calculate the freezing point and boiling point of a 0.55 m  CH3OH in water. (Kf = 1.8oCkg/mol;  kb= 0.51 oC kg/mol).

Which statement below is generally true regarding factors that affect the solubility of solids in water? O As the pressure increases, the solubility increases. O As the pressure increases, the solubility increases. O lons with greater charge are more soluble in water. O Nonpolar solids are more soluble in water than polar solids.

✓mall amount of acetonitrile (CH₂CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) CH₂CN 98 B H₂O Use these sketches to answer the questions in the table below. The enthalpy of solution AH soln is negative when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage A to B? What force would oppose or favor the system moving from Stage A to B? Check all that apply. 0 O absorbed O released O neither absorbed nor released none Olonic bonding force O covalent bonding force metal bonding force Ohydrogen-bonding force dipole force ion-dipole force Odispersion force 0.0. X solution. S