1. What is the boiling point of a 3.0 m Ca(NO3)2 solution in water?
Where:
the change in boiling point (ΔTb) = mKb
m is the molality of the solution
Kb (the boiling point constant) for water is 0.512
2. The freezing point of ethanol (C2H5OH) is -114.6 °C. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin a nonelectrolyte) in 200.0 g of ethanol?
Where:
ΔTf = mKf
The molal freezing point depression constant (Kf) ( for ethanol is 2.00 °C/m.
3. The osmotic pressure of blood is 7.65 atm at 37°C. If blood were considered a solution of NaCl, what is the molar concentration of NaCl in blood? Assume an ideal van’t Hoff factor.
Where:
Π = iMRT
R is the ideal gas law constant ( 0.08205 L ⋅ a t m m o l ⋅ K)
and T is the absolute temperature
4. Why do ice cubes get smaller when left in the freezer for a long time?
Neither The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps nor The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase accurately explain why ice cubes get smaller in the freezer over time.
The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps.
The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase.
Both The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps and The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase occur.
5. What volume of 18.0 M sulfuric acid is required to prepare 26.20 L of 0.126 M H2SO4?
3.30 L
207.94 mL
0.183 L
471.60 mL
5.45 mL
1. What is the boiling point of a 3.0 m Ca(NO3)2 solution in water? Where: the...
4. Why do ice cubes get smaller when left in the freezer for a long time? Neither The ice cubes melt during the brief warming cycles of auto-defrost and freezer access, thus leaving the ice cubes smaller and making them stick together in clumps nor The water molecules of the ice sublime from the solid to gaseous phase without ever entering a liquid phase accurately explain why ice cubes get smaller in the freezer over time. The ice...
8. What is the final boiling point of a 1.25 molal solution of sugar in water? The Kb for water is 0.512 C/m. (For sugar i = l.) 9. A solution was prepared by dissolving 0.52 mol hexane into 400g CCl4. What is the change in freezing point of this solution? Carbon tetrachloride has a freezing point depression constant of 29.8 Cm,and freezes at-23。. 10. A solution was prepared by dissolving 0.26 moles of ethanol (C2HsOH) into 750g Diethyl ether....
0/5pts Incorrect Question 18 What is the boiling point of a 3.0 m Ca(NOs)2 solution in water? Where the change in boiling point (AT)-mk wmis the molality of the solution K (the boiling point constant) for water is 0.512 104.6
The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 12.54 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 158.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C....
T/F (1) Additives added to ethanol will have the same effect on boiling point as the same amount of additives added to water Ethanol changes its solution boiling point with additive mass fraction of 0.15 more than water changes its boiling point with a mass fraction of 0.25 If the activity coefficient of solute A in a solution is equal to 1, A has little to no preference to other molecules around it in solution It is likely that flavors...